Problem: A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 55.6 mL 0.200 M HNO3.

FREE Expert Solution

▪ HNO3 → strong acid
▪ NaOH → strong base
▪ the reaction between a strong base and strong acid → no need to create an ICE chart

Balanced reaction:              HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3(aq)



Step 1: Calculate the initial amount (in moles) of the acid and base

Recall:

molarity (M)=molL

moles HNO3=0.200 mol HNO3L 55.6 mL x 10-3 L1 mL

moles HNO3 = 0.0112 mol

moles NaOH=0.200 mol NaOHL50.0 mL x 10-3 L1 mL

moles NaOH = 0.0100 mol


The amount of HNO3 is greater than NaOH, therefore there will be HNO3 left after the reaction


Step 2: Calculate the amount of HNO3 reacted

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Problem Details

A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 55.6 mL 0.200 M HNO3.


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