Chemistry

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

2 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.

    [tex]pH=-\log [H^+][/tex]

    [tex]pH=log\frac {1}{H^+}[/tex]

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

    1. Solution A has a pH of 3

    [tex]13=-log[H^+][/tex]

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

    2. solution Z has  a pH of 6.

    [tex]16=-log[H^+][/tex]

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

    Thus Solution A with low pH has higher [tex]H^+[/tex] concentration.

    [tex]\frac{H^+_A}{H^+_Z}=\frac{10^{-13}}{10^{-16}}=10^3=1000[/tex]

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