For a 0.16 M solution of HCl, calculate: [H+], pH, pOH, and [OH-] Omit molarity

Question

For a 0.16 M solution of HCl, calculate: [H+], pH, pOH, and [OH-] Omit molarity units from your answers and determine all pH and pOH values to two decimal places. To enter an answer in scientific notation: 1.2 x 10-4 = 1.2E-4 [H+]= pH= pOH= [OH-]= Now make the same calculations for a 1.0 x 10-12 M solution of HBr. [H+]= pH= pOH= [OH-]=

Explanation / Answer

HCl -> H+ + Cl- 0.16M Hcl produce 0.16M of H+ so [H+] = 0.16M pH = -log(0.16) = 0.80 [H+][OH-] = 10^-14 so [OH-] = 10^-14 / 0.16 = 6.25 x 10^-14M = 6.25E-14 so Poh = -log( 6.25 x 10^-14) = 13.204

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