5) Calculate [H*] for each of the following solutions, and indicate whether the

Question

5) Calculate [H*] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. (a) [OH] 0.00054 M (b) a solution in which [OH] is 100 times greater than [H] If NaOH is added to water, how does [H] change (increases/decreases)? How does pH change (increases/decreases)? 6) 7) Complete the following table by calculating the missing entries. In each case, indicate whether the solution is acidic or basic. pH pOH OT Acidic or basic? 4.24 1.80 6.2x1010 M 8.2×102 M 8) Calculate the pH of each of the following strong acid solutions. (a) 0.0274 M HNO3 (b) 0.792 g of HCIOs in 2.52 L of solution

Explanation / Answer

5)

a)

[OH-] = 0.00054 M

[H+] [OH-] = Kw

[H+] x 0.00053 = 1.0 x 10^-14

[H+] = 1.85 x 10^-11 M

pH = -log (H+) = -log (1.85 x 10^-11)

pH = 10.73

here pH > 7 . so

this solution is basic

b)

[OH-] = 100 x [H+]

[H+] x [OH-] = 1.0 x 10^-14

[H+] x 100 x [H+] = 1.0 x 10^-14

[H+]^2 = 1 x 10^-16

[H+] = 1.0 x 10^-8 M

pH = 8

so this is also basic solution

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