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Dennis_Churaev [7]
4 years ago
11

Plz answer correctly....The concentration of either the H+ ion or the OH − ion is given for four aqueous solutions at 298 K.?

Chemistry
2 answers:
olga2289 [7]4 years ago
6 0

Explanation :

Solution for part (a) :

Concentration of H^+ = 8.0\times 10^{-13}M

As we know that,

[H^+][OH^-]=10^{-14}

Now put the value of concentration of hydrogen ion, we get concentration of hydroxide ion.

(8.0\times 10^{-13})\times [OH^-]=10^{-14}

[OH^-]=1.25\times 10^{-2}M

From this we conclude that, the concentration of hydroxide ion is more than the hydrogen ion that means the solution is basic in nature.

Solution for part (b) :

Concentration of OH^- = 4.0\times 10^{-7}M

As we know that,

[H^+][OH^-]=10^{-14}

Now put the value of concentration of hydroxide ion, we get concentration of hydrogen ion.

[H^+]\times (4.0\times 10^{-7})=10^{-14}

[H^+]=0.25\times 10^{-7}M

From this we conclude that, the concentration of hydrogen ion is more than the hydroxide ion that means the solution is acidic in nature.

Solution for part (c) :

Concentration of OH^- = 5.0\times 10^{-3}M

As we know that,

[H^+][OH^-]=10^{-14}

Now put the value of concentration of hydroxide ion, we get concentration of hydrogen ion.

[H^+]\times (3.0\times 10^{-3})=10^{-14}

[H^+]=0.25\times 10^{-7}M

From this we conclude that, the concentration of hydroxide ion is more than the hydrogen ion that means the solution is basic in nature.

Solution for part (d) :

Concentration of H^+ = 8.0\times 10^{-5}M

As we know that,

[H^+][OH^-]=10^{-14}

Now put the value of concentration of hydrogen ion, we get concentration of hydroxide ion.

(8.0\times 10^{-5})\times [OH^-]=10^{-14}

[OH^-]=1.25\times 10^{-2}M

From this we conclude that, the concentration of hydrogen ion is more than the hydroxide ion that means the solution is acidic in nature.

Rudiy274 years ago
4 0

Definitions needed:  

pH = -log[H^+]  

pOH = -log[OH^-]  

pH + pOH = 14  

[H^+]*[OH^-] = 10^-14  

(a) [H+] = 3.0 10-13 M  

[OH ‾ ] = _____ M  

Acidic, Basic, or Neutral?  

[H^+]*[OH^-] = 10^-14  

[OH^-] = (10^-14)/[H^+]  

[OH^-] = (10^-14)/(3.0 10-13 M) = 0.033 M  

That's a high concentration of [OH^-], so the solution is basic  

(b) [OH ‾ ] = 3.0 10-7 M  

[H+] = ______M  

Acidic, Basic, or Neutral?  

[H^+]*[OH^-] = 10^-14  

[H^+]* = (10^-14)/[OH^-]  

[H^+]* = (10^-14)/(3.0 10-7 M) = 3.33 x 10^-8  

That would be a slightly basic solution (pH just higher than 7).

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