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Calculate the concentration of H+ ions in a 0.010M aqueous solution .pdf

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Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M Solution Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M.

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Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M Solution Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M

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Calculate the concentration of H+ ions in a 0.010M aqueous solution .pdf

  • 1. Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M Solution Calculate the concentration of H+ ions in a 0.010M aqueous solution of sulfuric acid. Note that H2SO4 is a strong acid initially H2SO4 = H+ + HSO4- [H+] = 0.01 M and [HSO4-] = 0.01 HSO4- is a weak acid so HSO4- <=> H+ + SO4-2 Ka2 = 1.2*10^-2 so Ka2 = [H+][SO4-2]/[HSO4-] 1.2*10^-2 = (0.01+x)(x)/(0.01-x) solve for x 0.012 = (0.01+x)(x)/(0.01-x) 0.012*0.01 - 0.012x = 0.01x + x^2 x^2 + 0.022x - 0.00012 = 0 x = 0.004524 [H+] = 0.01 + 0.004524 = 0.014524 M