Answered

Solution A has a pH of 3 and solution Z has

a pH of 6. How many times greater is the

hydronium ion concentration in solution A than

the hydronium ion concentration in solution Z?

(1) 100 (3) 3

(2) 2 (4) 1000

Verified Answer :

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: (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.

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

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