Question

Solution A has a pH of 3 and solution Z has

Answer 1

PH of a solution is -ln[H3O+] so,in case of A pH=3 or,-log[H3O+]=3 or,[H3O+]=10^-3 in case of B pH=6 pr,-log[H3O+]=6 or, [H3O+]=10^-6 so,hydronium ion concentration in solution A /the hydronium ion concentration in solution Z =10^-3/10^-6 =1000 2) Ca(OH)2+2 HNO3=Ca(NO3)2+2 H2O so the answer is 2.

Answer 2

Answer: (4) 1000

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

$pH=-\log [H^+]$

$pH=log\frac {1}{H^+}$

Thus as pH and $H^+$ are inversely related, a solution having lower pH will have more amount of $H^+$ concentration. And a solution having more pH will have less amount of $H^+$ concentration.

1. Solution A has a pH of 3

$13=-log[H^+]$

$[H^+_A]=10^{-13}$

2. solution Z has  a pH of 6.

$16=-log[H^+]$

$[H^+_Z]=10^{-16}$

Thus Solution A with low pH has higher $H^+$ concentration.

$\frac{H^+_A}{H^+_Z}=\frac{10^{-13}}{10^{-16}}=10^3=1000$