Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :
a. $60 mL\dfrac{M}{10}HCL+40 mL\dfrac{M}{10} NaOH$
b. $55 mL\dfrac{M}{10}HCL+45 mL\dfrac{M}{10} NaOH$
c. $75 mL\dfrac{M}{5}HCL+25 mL\dfrac{M}{5} NaOH$
d. $100 mL\dfrac{M}{10}HCL+100 mL\dfrac{M}{10} NaOH$
pH of which one of them will be equal to 1?
d
a
b
c
Explanation:
• Meq of HCl = $75\times\dfrac{1}{5}\times1=15$
• Meq of NaOH = $25\times\dfrac{1}{5}\times1=5$
• Meq of HCl in resulting solution = 10
• Molarity of $[H^+]$ in resulting mixture
$\dfrac{10}{100}=\dfrac{1}{10}$
$pH=-log\left[H^+\right]=log \left[\dfrac{1}{10}\right]=1.0$
• Meq of HCl = $75\times\dfrac{1}{5}\times1=15$
• Meq of NaOH = $25\times\dfrac{1}{5}\times1=5$
• Meq of HCl in resulting solution = 10
• Molarity of $[H^+]$ in resulting mixture
$\dfrac{10}{100}=\dfrac{1}{10}$
$pH=-log\left[H^+\right]=log \left[\dfrac{1}{10}\right]=1.0$
