• Dmg Hcl Rda
• Dmg Hcl Good For
• Dmg Hcl Optimal Daily Intake
• Dmg Hcl Interactions

Dimethylglycine (DMG) is a derivative of the amino acid glycine with the structural formula (CH 3) 2 NCH 2 COOH. It can be found in beans and liver. It can be formed from trimethylglycine upon the loss of one of its methyl groups. It is also a byproduct of the metabolism of choline.

HCL utilizes transformational tools, modules, networks and solutions to empower the width of the talent base. Signature learning suites, residential programs and role-ready skill development are designed to transform prospects into highly capable professionals with all the right skill-sets and certifications. DMG is an organic compound which is sparingly soluble in water, and thus, the solution is prepared in ethanol. Excess of DMG is added to the solution containing Ni. However, too much excess of reagent is not preferred. The reason behind this is: If excess DMG is added.

[Last updated 14th August, 2018]

Betaine HCl is a supplement linked with many health claims.

In particular, improving poor digestion from low stomach acid.

But are these claims backed by science? Is it safe and effective?

This article explores the current evidence for betaine HCl supplementation.

Contents

What is Betaine HCl?

Betaine hydrochloride (HCl) is a dietary supplement made from a combination of betaine and hydrochloric acid.

Betaine (also called trimethylglycine) is found in certain foods and is also a product of choline metabolism.

Chemical structure of betaine. Image Source

Hydrochloric acid (HCl) is a very strong acid that is naturally produced by the stomach. It’s important in both digestion and immunity.

It’s mainly used by natural health practitioners as a treatment for digestive issues.

It comes in pill form and is sometimes combined with a digestive enzyme called pepsin.

For the record, Betaine HCl should not be confused with betaine anhydrous. Betaine anhydrous is a drug that is FDA-approved to treat homocystinuria and potentially liver disease.

FDA Regulations

Note that Betaine HCl is a supplement, not a drug.

That means it’s not regulated by the FDA and there are no standards for usage and dose.

In fact, The FDA doesn’t recognize over-the-counter drugs that contain betaine HCl as safe or effective.

Still, personal testimonies and online reports suggest that it’s helpful for various medical conditions.

This article will focus specifically on betaine HCl.

Summary: Betaine HCl is a supplement made from betaine and hydrochloric acid. It’s used by natural health professionals to treat various digestive issues. Betaine HCl is not regulated by the FDA.

Betaine HCl and Hypochlorhydria

Betaine HCl is said to help remedy hypochlorhydria.

Hypochlorhydria refers to when the stomach is not as acidic as it should be. An acidic stomach is very important for both healthy digestion and immunity (1, 2).

Stomach acidity is measured by a term called pH, with a low pH indicating an acidic environment, and high pH indicating an alkaline environment.

The pH scale. Lower numbers indicate greater acidity, while higher numbers indicate increasing alkalinity. Image source

The rise in pH seen in hypochlorhydria results from a low concentration of hydrochloric acid in the stomach’s gastric juice. Similarly, achlorhydria is a complete lack of HCl in the gastric juice (1).

Betaine HCI May Only Help Temporarily

As betaine HCl contains hydrochloric acid, it’s been said to improve digestive function and other conditions that stem from weak stomach acid.

However, low stomach acid is most often a symptom of another health problem, rather than a disease itself. As you would expect then, betaine HCl does appear to restore stomach acidity somewhat… but only temporarily.

In one study of 6 healthy adults with drug-induced hypochlorhydria, a single 1500 mg dose of betaine HCl significantly lowered gastric pH (increased acidity) within six minutes for all volunteers.

However, gastric pH of all subjects returned to previous levels in just under two hours (3).

Another study found similar results. Betaine HCl was effective in lowering gastric pH within an average of 12 minutes for 10 healthy volunteers. Stomach pH returned to previous levels within 69 minutes, on average (4).

As such, the best way to permanently restore a healthy stomach pH would be to treat the underlying cause.

Common causes of hyperchlorhydria include H. pylori bacteria and atrophic gastritis. Long-term use of acid-reducing drugs, including H2-receptor agonists and proton-pump inhibitors (such as Omeprazole for reflux) are also a risk factor.

HIV, gastric bypass surgery, and certain autoimmune conditions have also been shown to lower stomach acid (5, 6, 7, 8).

Summary: Betaine HCl is said to correct low stomach acid (hypochlorhydria), which is linked to several digestive and immune conditions. However, research indicates it only helps temporarily.

Betaine HCl, Acid Reflux, and Functional Dyspepsia

Acid reflux is a common condition in which gastric acid moves upward from the stomach into the esophagus.

Most people have experienced it at least once. Frequent episodes of reflux are symptomatic of gastroesophageal reflux disease (GERD), gastroparesis or functional dyspepsia.

A comparison of the lower esophageal sphincter in a healthy adult and an adult with GERD. Image Source

Proponents of betaine HCl argue that food breaks down in the stomach more slowly when stomach acid is inadequate. This means food sits in the stomach longer (slower stomach emptying), creating upward pressure on the lower esophageal sphincter and causing reflux.

Small studies have found stomach emptying to be especially slow in those with hypochlorhydria. And there does appear to be links between delayed stomach emptying, GERD, and functional dyspepsia (9, 10, 11).

However, studies have not been able to establish hypochlorhydria as a direct cause of GERD or functional dyspepsia. This may be because many factors can contribute to GERD or dyspepsia in the same person.

Additionally, these conditions can also exist with normal stomach acid levels (11).

Aside from case studies, betaine HCl hasn’t been studied as a therapy for acid reflux or GERD (12, 13).

Until there is more solid research – or unless your doctor recommends it – betaine HCl is not recommended for reflux or dyspepsia.

Summary: There’s indirect evidence that hypochlorhydria may contribute to reflux and functional dyspepsia. However, there is no research that indicates betaine HCl is useful in treating either condition.

Betaine HCl and Drug Absorption

Certain medications are less effective if the stomach is too acidic or too alkaline (14).

Some of the strongest research in support of betaine HCl relates to medication absorption in those with hypochlorhydria.

One such drug is dasatinib, an oral chemotherapy medication used in chronic myeloid leukemia that is best absorbed at a pH of 6.0 or lower. Antacids and H₂ blockers have been shown to reduce dasatinib absorption by up to 60% (4, 15).

By contrast, betaine HCl has been shown to markedly improve dasatinib. In a study of 10 healthy adults taking acid-reducing medications, each subject participated in 3 separate treatments:

• Treatment A was 100 mg of dasatinib alone.
• For Treatment B, volunteers took 20 mg of the proton pump inhibitor rabepazole twice per day until gastric pH was greater than 4.0. Then, they received a 100 mg dose of dasatinib.
• For Treatment C, volunteers took 20 mg of rabepazole twice per day until gastric pH was greater than 4.0. Then, they received a 1500 mg dose of betaine HCl, followed 5 minutes later by a 100 mg dose of dasatinib.

Dasatinib absorption for Treatment B was 92% lower than it was for Treatment A. But betaine HCl supplementation resulted in a 15-fold increase in drug absorption compared to Treatment B.

Additionally, drug absorption for Treatment C was 5% higher than Treatment A, which suggests that betaine HCl could slightly boost the effectiveness of dasatinib in the absence of hypochlorhydria (4).

A comparison of dasatinib absorption taken alone, after pretreatment with rabepazole, and using betaine HCl after pretreatment with rebepazole. Higher concentration indicates better drug absorption.

However, these results should be interpreted with caution as the study was small and chemotherapy absoprtion is influenced by so many factors.

Betaine HCl hasn’t been studied with other drugs to date. It would be interesting to see its effects on other pH-dependent drugs, such as the HIV drug ataznavir or certain antibiotics (16, 17).

Summary: Small studies have shown that betaine HCl improves absorption of the chemotherapy drug dasatinib in healthy volunteers with drug-induced hypochlorhydria. It hasn’t been studied on the absorption of other drugs.

Betaine HCl and Nutrient Absorption

Low stomach acidity has been linked to impaired absorption of several nutrients.

These include iron, vitamin B12, magnesium, vitamin C, and calcium (18, 19, 20, 21).

Supplements or other treatments that restore acid balance could be helpful, at least in theory.

Unfortunately, there’s no studies on betaine HCl and nutrient deficiencies. All claims are based on patient testimonials (reports). Until there is at least some evidence, it should not be recommended to enhance nutrient absorption.

Additionally, a vitamin or mineral deficiency often results from an underlying medical condition or lifestyle issue. The cause should be addressed rather than masked with betaine HCl (which may or may not help.)

Also keep in mind that the deficiencies mentioned above also occur in people with normal gastric pH, which supports the idea that low gastric pH is a symptom of something else (22).

Summary: Low stomach acid has been linked with deficiency of certain vitamins and minerals. Patient testimonials suggest that betaine HCl helps improve nutrient absorption, but there’s no scientific evidence to support these claims.

Do You Need a Betaine HCl Supplement?

Some health bloggers argue that most adults should supplement with betaine HCl.

Many of these claims come from two specific studies. One commonly cited study suggests that 20-50% of adults ages 65 and older are deficient in stomach HCl.

But this figure is actually the estimated prevalence of Americans with atrophic gastritis, not specifically hypochlorhydria. There’s some question as to the prevalence of atrophic gastritis, especially worldwide (23, 24).

The second study was published in 1967. Of 3484 volunteers, 27% were found to have achlorhydria (25).

But the methods for this study have since been called into question due to high potential for inaccuracy (26, 27).

Two non-invasive home tests for low stomach acid have been proposed. One involves drinking a mixture of baking soda and water and measuring how long it takes to belch. The second involves a trial of betaine HCl supplements

These methods haven’t been validated by studies and could even be dangerous for those with certain medical conditions.

Overall, we simply don’t have enough direct evidence to know if betaine HCl is useful or safe, of if hypochlorhydria is even a common problem.

Summary: Many health bloggers have argued that most adults would benefit from betaine HCl supplements. But no strong studies support these claims. More evidence is needed.

Betaine HCl Supplements and Digestion

Betaine HCl has become very popular among health bloggers, with many recommending it widely.

To be fair, some of these arguments about stomach acid are interesting and thought-provoking. But studies on betaine HCl are incredibly sparse.

Aside from case studies, no scientific evidence supports claims that betaine HCl will cure reflux and other digestive ailments.

In fact, it’s only been shown to restore acid balance in those taking acid-reducing drugs, and to boost absorption of certain pH-dependent drugs.

More importantly:

• Betaine HCl isn’t generally recognized as safe and effective by the FDA.
• Hypochlorhydria usually isn’t a disease in and of itself, but rather a symptom of an underlying medical

Overall, betaine HCl supplements are not worth your money, except for those taking them under a doctor’s supervision.

pH

The pH = - log [H₃O]⁺ is a measure of the hydronium concentration of an aqueous solution. The lower the pH the more acidic the solution. A table summarizing log values for various powers of ten is shown below.

A 0.1 M HCl solution has 0.1 M H₃O⁺ and a pH = 1, whereas a 0.1 M acetic acid solution (CH₃COOH) has 0.001 M H₃O⁺ (since it is only 1% dissociated) and a pH = 3

The K_eq of an acid is a measure of the strength of an acid. For the general acid reaction with water:

HA(aq) + H₂O(l) <> H₃O⁺ + A^-, K_eq = ([H₃O⁺][A^-])/([HA][H₂O])

For a strong acid, K_eq > 1 and for a weak acid, K_eq < 1.

[H₂O] is approximately 55.5 M in a diliute acid solution, and is essentially constant (since it is present in such great excess). Hence K_eq[H₂O] = ([H₃O⁺][A^-])/[HA] = K_a.

K_a, the acid constant,is also a constant; for a strong acid, K_a > 1 and for a weak acid, K_a < 1

Consider the two reactions below in which the concentration of HCl and CH₃COOH are each 0.1 M.:

HCl + H₂O ----------> H₃O⁺ + Cl^-

Dmg Hcl Rda

At equilibrium, [H₃O⁺] and [Cl^- ] are both approximately 0.1 M and HCl is effectively 0. In actuality, some HCl is left and can be shown to be 0.000000001 M = 10^-9 M.
Hence K_a = ([H₃O⁺][A^-])/[HA] = (10^-1)(10^-1)/10^-9 = 10⁷ >> 1.

CH₃COOH + H₂O ----------> H₃O⁺ + CH₃COO^-

At equilibrium, [H₃O⁺] and [Cl^- ] are both approximately 0.001 M and CH₃COOH is 0.099 M = 9.9 x10^-2 M.
Hence K_a = ([H₃O⁺][A^-])/[HA] = (10^-3)(10^-3)/9.9 x 10^-2 = 1.01 x 10^-5 << 1.

Just as pH = -log[H₃O]⁺, pK_a = -logK_a. In the above examples, the pK_a of HCl is -7 while that of acetic acid is approx. 5.

The pK_a of an acid is a measure of the strength of an acid. It is a constant and does not depend on the concentration of the acid. The lower the pK_a, the more stronger the acid.

Water can act as both a weak acid and a weak base. It can interact with itself to form the hydronium and hydroxide ion, as shown below:

H₂O + H₂O ----------> H₃O⁺ + OH^-

In pure water, [H₃O⁺] and [OH^-] are equal (as seen in the equation above) and are each 1x10^-7 M. Hence the pH of neutral water is 7.0

Buffers

Buffer solutions consist of weak acids and salts of weak acids.They can be created by mixing a solution of a weak acid (such as acetic acid) with a solution of a salt of a weak acid (such as sodium acetate). Alternatively, buffer solutions can be created by partially titrating a solution of a weak acid with sodium hydroxide which neutralizes part of the acid to form the salt of the weak acid, with the sodium ion provided by the added titrant.

Dmg Hcl Good For

Buffer solutions can neutralize the addition of small amounts of an acid (which reacts with the base product of the weak acid) and small amounts of a base (which reacts with the weak acid).

Consider what would happen to the pH of pure water (pH = 7) if either 0.01 mol of NaOH or 0.01 mol of HCl were added to sufficient water to make 1L. The first solution would now have an [OH^-] = 0.01 M and hence a [H₃O⁺] = 1 x 10^-12 M, or a pH = 12. The second solution would have a [H₃O⁺] = 1 x 10^-2 M, or a pH = 2. This examples shows that the addition of a small amount fo either acid or base to water dramatically changes the pH. Consider the pH of pure water to be like a balance. Addition of small amounts of either acid or bases dramatically changes the balance (pH)

Now consider what would happen to the pH of a 0.5 M acetic acid (a weak acid) solution but which also contains 0.5 M sodium acetate (a salt of a weak acid). (Recipe: 5.8 ml glacial AA + 17.6 g NaAc.3H20 to 200 ml total)

The appropriate equation to describe this solution is:

CH₃COOH + H₂O <> H₃O⁺ + CH₃COO^-

The pH of the solution can be calculate if you know the K_a of acetic acid = 1.8 x 10^-5. Plug this into the following equation to get x = [H₃O⁺] and pH as follows:

K_a = ([H₃O⁺] [CH₃COO^-])/[CH₃COOH] = x(0.5)/0.5 = 1.8 x 10^-5

x = [H₃O⁺] = 1.8 x 10^-5; pH = 4.74

Now if 0.01 mol of NaOH was added (without changing the volume), the hydroxide would react with the weak acid as shown below:

CH₃COOH + OH^- <> H₂O + CH₃COO^-

Therefore the base is consumed, CH₃COOH is reduced to 0.49 M and CH₃COO^- increases to 0.51. As above, x can be calculated and the pH determined.

K_a = ([H₃O⁺] [CH₃COO^-])/[CH₃COOH] = x(0.51)/0.49 = 1.8 x 10^-5

x = [H₃O⁺] = 1.72 x 10^-5; pH = 4.76.

The pH was raised only by 0.02 units in comparison to the case of pure water whose pH increased by 5 units.

Now if 0.01 mol of HCl was added (without changing the volume), the HCl would react with the weak base acetate as shown below:

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HCl + CH₃COO^- <> Cl^- + CH₃COOH

Therefore the added HCl is consumed, CH₃COO^- is reduced to 0.49 M and CH₃COOH increases to 0.51. As above, x can be calculated and the pH determined.

K_a = ([H₃O⁺] [CH₃COO^-])/[CH₃COOH] = x(0.49)/0.51 = 1.8 x 10^-5

x = [H₃O⁺] = 1.87 x 10^-5; pH = 4.73. The pH was reduced only by 0.01 units in comparison to the case of pure water whose pH dropped by 5 units.

Biological Buffer Systems:

pH in the body has to be very tightly controlled. Specifically, the pH of blood and intracellular spaces can not very much without serious consequences. Two common buffers systems are

• the H₂PO₄^- (weak acid) and HPO₄^2- (its base)
• H₂CO₃ - carbonic acid (weak acid) and HCO₃^- - bicarbonate (its base)

The later is most important in blood, which is maintained within a narrow range of 7.35-7.45. This buffer system is a bit more complicated since another reaction of carbonic acid must be considered - namely the breakdown of carbonic acid to water and CO₂.

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)

I demonstrated the reversible formation of carbonic acid in class by blowing into a water which was made slightly alkaline by the addition of a small amount of ammonia. The solution become more acidic, as indicated by the change of color of the solution when phenopthalein was added. The reaction of carbon dioxide with water to form carbon dioxide can be visualized below:

The two major components of the buffer system of blood are controlled by two different mechanisms:

H₂CO₃ is controlled by changing the respiration rate. If you breath more quickly and deeply (like when you hyperventiallate), you exhale more CO₂. This will decrease the blood carbonic acid by as shown in blue below. CO₂ concentrations decrease, pulling the equilibria below to the left which decreases H₃O⁺(aq)

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)

HCO₃^-(aq) (bicarbonate) is controlled by the rate at which it is excreted by the urine.

What happens to the blood pH when the relative amounts ofH₂CO₃(aq) and HCO₃^-(aq) change. Lets examine the Ka for the red part of the equation below, considering carbonic acid as a weak acid.

Dmg Hcl Optimal Daily Intake

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)

K_a = ([H₃O⁺][HCO₃^-])/[H₂CO₃] which can be rearranged to

[H₃O⁺] = K_a[H₂CO₃] /[HCO₃^-]. From this is should be clear that:

• if either [H₂CO₃] increases or [HCO₃^-] decreases or both, [H₃O⁺] increases and the pH decreases. If this decrease in pH is outside of the normal range, the condition is called acidosis.
• if either [H₂CO₃] decreases or [HCO₃^-] increases or both, [H₃O⁺] decreases and the pH increases making the blood more basic or alkaline. If this increase in pH is outside of the normal range, the condition is called alkalosis.

Two kinds of acidosis are common - respiratory acidosis and metabolic acidosis.

Metabolic acidosis: This occurs often in burn patients. Blood plasma leaks into damaged areas which can decrease total blood volume and flow, decreasing oxygen availability. This will increase anaerobic metabolism, just as when you are running a fast race and are deprived of oxygen. Lactic acid builds up in the blood, increasing the H₃O⁺ in the blood, shifts the equilibrium shown in red below to increase carbonic acid and decrease bicarbonate:

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)

This decreased pH causes the injured person to break harder to get rid of CO₂, which by Le Chateliers principle causes a helpful decrease in carbonic acid as shown in blue below:

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)

If the damage is to great so the person can't breath well, shock can develop.

Respiratory acidosis: This occurs in burn victims who have inhaled much smoke and can't breath well. Likewise it occurs in pulmonary diseases such as emphysema or a physical obstruction which hinders respiration. This causes CO₂ to build up, increasing carbonic acid and decreasing blood pH as shown below in red:

Dmg Hcl Interactions

CO₂(g) + H₂O(l) <> H₂CO₃(aq) + H₂O(l) <> H₃O⁺(aq) + HCO₃^-(aq)