Question

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

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

Step-by-step 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.

`(H^+_A)/(H^+_Z)=(10^(-13))/(10^(-16))=10^3=1000`