How many grams of nitric acid would be dissolved in 10.0mL of a nitric acid solution with a pH of 0.137?
step 1) convert given pH to concentration of [H3O^+]
10^-0.137 = 10^log[H3O^+] =
0.73M = [H3O^+]
Step 2) convert 10.0mL HNO3(nitric acid) to Liters. 10.0ml x 1L/1000mL = 0.0100L
step 3) multiply Molarity of H3O^+ times liters to get moles of Nitric acid.
0.73mol HNO3l/L x 0.0100L = 0.0073 mol HNO3 or 7.3x10^-3 mol HNO3
step4) moles to grams HNO3
0.0073 mol HNO3 x 63.01g HNO3/1 mol HNO3 = 0.46g HNO3(2 sig figs)