[H+] M [OH-] M ph poh
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1 ph and poh Name: Date: Period: 1. What is ph a measure of? 2. What is the equation used for finding ph? 3. What is the equation that relates to ph and poh? 4. Complete the following table: (first one is done as an example) [H+] M [OH-] M ph poh 5. What would be the ph of each of the following? a) M HCl g) M HCl b) M HNO3 h) M KOH c) M NaOH i) M HCl d) M HCl j) M HCl 6. Classify each of the following as acidic, neutral, or basic: Acidic, base, neutral a. 1.0 x x Acidic b. 1.0 x 10-5 c d e f g h i. 3.2 x 10-3 j. 1.8 x k l m n o p a) Tomatoes-4.2 b) soil-5.5 c) Eggs-7.8 d) milk-6.4 e) ammonia-11.0
2 ph Calculations Find the ph of the following acidic solutions: Show work to receive full credit. Put a box around your final answer. Round ALL final numerical answers to 2 decimal places 1) A M solution of HCl (hydrochloric acid) ) A 0.09 M solution of HBr (hydrobromic acid) ) A 1.34 x 10-4 M solution of hydrochloric acid ) A x 10-6 M solution of HI (hydroiodic acid) ) A 7.98 x 10-2 M solution of HNO 3 (nitric acid) ) A solution containing 1 mole of hydrochloric acid in 12 L of water ) A solution containing 0.34 moles of nitric acid in 735 L of water ) A solution containing moles of hydrobromic acid in 1098 L of water ) A solution containing.0074 moles of hydrochloric acid in 660 L of water ) A solution containing grams of hydrochloric acid in 120 ml of water ) A solution containing 5.0 x 10-4 grams of hydrobromic acid in 1.2 liters of water ) A solution containing 4.5 grams of nitric acid in 2.3 liters of water ) A solution containing grams of hydrochloric acid in 792 ml of water. 1.92
3 14) A solution containing 1.00 grams of nitric acid in 100 ml of water ) A solution containing 1.1 grams of nitric acid in 8.7 liters of water ) A solution containing 5.6 grams of hydroiodic acid in 1.5 liters of water ) A solution containing 0.01 grams of hydrochloric acid in 10.7 liters of water ) A solution containing 6.7 grams of nitric acid and 4.5 grams of hydrochloric acid in 8,000 ml of water ) A solution containing 45 grams of nitric acid and 998 grams of hydrobromic acid in 150,000 L of water ) A solution containing 0.09 grams of HCl, 0.9 grams of HBr, 9.0 grams of HI, and 90.0 grams of HNO 3 in fifty liters of water. 1.52
4 ph practice Answer the following question regarding ph. Must show all work to receive full credit. Put a box around your final answer. Round all answers to two decimal places. 1) What is the ph and poh of a 1.2 x 10-3 HBr solution? ph: 2.9 poh: ) What is the ph and poh of a 2.34 x 10-5 NaOH solution? poh: 4.6 ph: 9.4 3) What is the ph and poh of a solution made by adding water to 15 grams of hydroiodic acid until the volume of the solution is 2500 ml? ph: 1.6 poh: ) What is the ph and poh of a solution that was made by adding 400 ml of water to 350 ml of 5.0 x 10-3 M NaOH solution? poh: 2.7 ph: ) What is the ph and poh of a solution with a volume of 5.4 L that contains 15 grams of hydrochloric acid and 25 grams of nitric acid? ph: 0.82 poh: ) A swimming pool has a volume of one million liters. How many grams of HCl would need to be added to that swimming pool to bring the ph down from 7 to 4? (Assume the volume of the HCl is negligible) 3545 grams (100.0 moles)
5 ph Review Problems Show work to receive full credit. Put a box around your final answer. Round ALL numerical answers to 2 decimal places 1) What is the molarity of a solution that has 450 grams of sodium chloride in 800 ml of water? 9.61 M 2) What is the molarity of a solution that contains 100 grams of iron (II) nitrate in 2.4 liters of water? 0.23 M 3) What is the ph of a solution that contains 2.4 x 10-5 moles of hydrobromic acid in 0.5 L of water? ) What is the ph of a solution that contains 25 moles of nitric acid dissolved in 5000 liters of water? ) What is the ph of a solution that contains grams of hydrochloric acid in 100 ml of water? ) What is an acid/base indicator used for? 7) Define titration : 8) In a few steps, describe how you would titrate a base of unknown concentration with an acid with concentration 1 M. 9) I did a titration where it took 50 ml of 0.10 M hydrochloric acid to neutralize 500 ml of a base with unknown concentration. Using this titration information, what was the concentration of the base? 0.01 M 10) I did a titration where it took 25.0 ml of 5 M NaOH to neutralize 1000 ml of an acid with unknown concentration. Using this information, what was the concentration of the acid? M
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