One brand of extra-strength antacid tablets contains 750 mg of calcium carbonate (100 g/mol) in each tablet. stomach acid is essentially a hydrochloric acid solution. is so much calcium carbonate really needed to neutralize stomach acid? calculate the volume of stomach acid with a ph of 1.0 that one of these tablets could neutralize, and compare that value with the normal volume of stomach fluid, which usually is about 100 ml. one tablet can neutralize ml of stomach acid at a ph of 1.0.

a. 75
b. 150
c. 250
d. 15
e. 7.5

One tablet can neutralize 150 mL of stomach acid at a pH of 1.0

Explanation:

Step 1: Data given

Mass of calcium carbonate = 750 mg = 0.75 grams

Molar mass of CaCO3 = 100 g/mol

pH = 1.0

Step 2: The balanced equation

2HCl  +  CaCO3 →  CaCl2  +  H2CO3

Step 3: Calculate molarity of HCl

pH = -log[H+] = 1

[H+] = 0.1 M = 0.10 mol/L

Step 4: Calculate moles of CaCO3

Moles CaCO3 = 0.75 grams / 100g/mol

Moles CaCO3 = 0.0075 mol

Step 5: Calculate moles of HCl

For 2 moles HCl we need 1 mol CaCO3 to produce CaCl2 and 1 mole of H2CO3

For 0.0075 moles of CaCO3 we have 2*0.0075 = 0.015 moles HCl

Step 6: Calculate volume of HCl

Volume = moles /molarity

Volume = 0.015 moles / 0.1 M

Volume = 0.15 L = 150 mL

One tablet can neutralize 150 mL of stomach acid at a pH of 1.0.

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explanation:

i think it is d. e because the next one is igneous.