# Question 9 of 12 40 40 points you have a solution

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Question 9 of 12 4.0/ 4.0 Points `You have a solution with [H ] = 1.7 x 10-5 M. What would be its pH?
A.0.22 B.5.20 C.10.20 Correct D.4.77 Answer Key: D Feedback: Good. pH is discussed in 14.9 Question 10 of 12 4.0/ 4.0 Points `Suppose you have a sample that has a low pH (acidic). What would be true of the [OH-]? Correct
Feedback: Good. See section 14.9 Part 3 of 3 - 3.5/ 10.0 Points Question 11 of 12 2.0/ 5.0 Points *Suppose you have 25.00 mL of phosphoric acid, and you do not know what it's concentration is. If you titrated it with a 0.733 M potassium hydroxide solution, and it took 39.50 mL of the base to neutralize the acid. what was the concentration of the phosphoric acid? Write the neutralization reaction, balance it, name the products THEN Solve the problem above. You must show all work to receive credit.
Feedback: Found in Ch. 14 Comment: Great job determining the balanced reaction. Now use it to solve the problem... Question 12 of 12 1.5/ 5.0 Points *Calculate the molarity (M) for each of these solutions--you must show all work in detail to receive credit: (a) 121.45 g of KOH in 100.0 mL, (b) 23.49 g of NH4OH in 150.0 mL, (c) 217.5 g of LiNO3 in 1.50 L, (d) 15.25 g of Pb(C2H3O2)2 in 50.0 mL A) 121.45 g KOH x 1 mol/56.1056=2.165 M=mols solut/L sol= 2.165/0.1=21.65 = M 100ml x .001 L/1ml=0.1 B) 23.49 NH4OH X 1mol/35.0458 150mlx 1L/.001=.15 Feedback: Concentrations of solutions is discussed in Ch. 13 Comment: Good job with part A. I can tell you know where you were going with part B.. you just needed to work through it. Did you run out of time? QUIZ 7 Part 1 of 3 - 20.0/ 20.0 Points