Question

If you would like to increased the pH of the stomach from 1.00 to 2.00 using an antacid table,how many grams of CaCo3 will be required to change the pH value? assume that you have a 1.00L stomach volume. (please type your answer) Thanks

Answer 1

According to Henderson–Hasselbalch equation

Buffer p^H = p^K_a + log [salt]/[acid]

p^H(1) = p^K_a + log [salt]₁/[acid]₁

p^H(2) = p^K_a + log [salt]₂/[acid]₂

p^H(2) - p^H(1) = log ([salt]₂/[acid]₂([acid]₁/[salt]₁

if we are changing the p^H by adding salt [acid]₁ = [acid]₂

p^H(2) - p^H(1) = log [salt]₂/[salt]₁

if we want to raise p^H of the stomach (carbonate buffer) from 1.00 to 2.00 by CaCo3 salt

2-1 = log [salt]₂/[salt]₁

[salt]₂/[salt]₁ = 10

we have raise the salt concentration by 10 times to increae p^H of 1 unit

If stomach volume is 1L we have to add 10 moles of CaCo3 to increased the pH of the stomach from 1.00 to 2.00

1000 g of CaCo3 is needed