1. Determine the pH (to two decimal places) of the solution that is produced by
ID: 922416 • Letter: 1
Question
1. Determine the pH (to two decimal places) of the solution that is produced by mixing 74.5 mL of 5.92×10-1 M HClO4 with 150 mL of 4.68×10-1 M HCl.
2. Determine the pOH (to two decimal places) of the solution that is produced by mixing 102 mL of 8.81×10-2 M MgO with 801 mL of 1.29×10-4 M Ca(OH)2.
3. Determine the pH (to two decimal places) of the solution that is produced by mixing 5.05 mL of 7.91×10-5 M HI with 7.73 mL of 8.38×10-5 M Mg(OH)2.
4. The pH of a 8.84×10-3 M solution of a weak monoprotic acid is 6.26. Calculate the percent dissociation of the acid to 3 significant figures.
5. The pH of a 3.26×10-3 M solution of a weak base that will accept only one proton is 9.51. Calculate the percent dissociation of the base to 3 significant figures.
Explanation / Answer
1. Determine the pH (to two decimal places) of the solution that is produced by mixing 74.5 mL of 5.92×10-1 M HClO4 with 150 mL of 4.68×10-1 M HCl.
Total H+ ions = mol of H from ClO4- and mol of H from HCl
mol of H ClO4- = M*V = 74.5*5.92*10^-1 = 44.104 mol of H+
mol of H+ Cl = M*V = 150*4.68*10^-1 = 70.2 mol of H+
Total H+ = 70.2+44.104 = 114.304 mol of H+
[H+] = mmol of H+ / ml
total ml = V1+V2 = 74.5+150 = 224.5 ml
[H+] = mmol of H+ / ml´= 114.304 /224.5 = 0.509149
pH = -log(H+) = -log(0.509149) = 0.29315
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