how many ml of 0.50 m naoh solution are required to completely titrate 15.0 ml of 0.20 m hno₃ solution?\na…

Explanation:

Step1: Write the balanced chemical equation

$HNO_3 + NaOH=NaNO_3 + H_2O$ The mole - ratio of $HNO_3$ to $NaOH$ is 1:1.

Step2: Use the formula $n = M\times V$

For $HNO_3$, $M_1 = 0.20\ M$ and $V_1=15.0\ mL$. So the number of moles of $HNO_3$, $n_1 = M_1\times V_1=0.20\ mol/L\times15.0\times10^{- 3}\ L = 3.0\times10^{-3}\ mol$. Since the mole - ratio of $HNO_3$ to $NaOH$ is 1:1, the number of moles of $NaOH$, $n_2=n_1 = 3.0\times10^{-3}\ mol$.

Step3: Calculate the volume of $NaOH$

For $NaOH$, $M_2 = 0.50\ M$. Using the formula $V=\frac{n}{M}$, we have $V_2=\frac{n_2}{M_2}=\frac{3.0\times10^{-3}\ mol}{0.50\ mol/L}=6.0\times10^{-3}\ L = 6.0\ mL$.

Answer:

A. 6.0 mL