Question

What volume of water must be added to 10.5 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0 g

Answer 1

Answer:

$V'=1040ml$

Explanation:

From the question we are told that:

Initial Volume $V_1=10.5mL$

Initial Aciditity of $HN0_3 pH_1=2.0g$

Finial Aciditity of $HN0_3 pH_2=4.0g$

Generally the equation for Acidity &Volume Relationship is mathematically given by

$N_1V_1=N_2V_2$

Therefore

$V_2=\frac{N_1V_2}{N_2}$

$V_2=\frac{10^{-2}*10.5}{10^{-4}}V_2=1050ml$

Therefore

Change in Water volume is

$V'=V_2-V_1$

$V'=1050ml-10ml$

$V'=1040ml$