A patient is suspected of having low stomach acid, a condition known as hypochlo

Question

A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 18.00 mL sample of her gastric juices and titrate the sample with 0.000186 M KOH. The gastric juice sample required 7.17 ml of the KOH titrant to neutralize it Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. Number For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia? O Yes O No Unable to determine

Explanation / Answer

ANS:

The acidity in the gastric juice is due to HCl acid.

Now using the formula , M1V1 = M2V2 , the molarity of acid can be determined.

Putting all the values we get :

0.000186 × 7.17 = M2 x 18.00

M2 = 0.04992 M

pH = -log[H+]

pH = -log[0.04992]

pH = 1.301

So the pH of gastric juice sample will be 1.301

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