# 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:

moles HNO3 = 0.0112 mol

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

93% (32 ratings) ###### 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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What scientific concept do you need to know in order to solve this problem?

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