Test%203%20Practice

Test 3 Practice - NH 3 NO 3 K b(CH 3 NH 2 = 4.4 10 −6 Test 3 Practice 10 Classify the salt CH 3 NH 3 NO 2 as acidic basic or neutral(see question

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Test 3 Practice Strong Acids 1. Solve for the [H 3 O + ] and pH of 0.45 M NaOH. Weak Acids 2. Solve for the pH of 0.23 M HClO with K a = 2.9 * 10 −8 3. Solve for the %diss above Buffers 4. Solve for the pH of a buffer made of 1.00 L of 0.10 M HNO 2 and 0.10 M NO 2 . The K a of HNO 2 = 7.10 * 10 −4
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Test 3 Practice 5. Solve for the pH of the above buffer after 1.00 g of NaOH are added. 6. Solve for the pH of 1.000 L of pure water with 1.00 g of NaOH added. Neutralization reactions 7. Write a neutralization reaction for HCl with NH 3 . Predict if this reaction would favor the reactants or the products. Salts 8. Solve for the pH of 0.100 M NaNO 3 . 9. Solve for the pH of 0.50 M CH 3
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Unformatted text preview: NH 3 NO 3 K b (CH 3 NH 2 = 4.4 * 10 −6 ) Test 3 Practice 10. Classify the salt CH 3 NH 3 NO 2 as acidic, basic or neutral (see question above and K a (HNO 2 ) = 7.1 * 10 −4 ) 11. Given that 25.0 g of Zn(IO 3 ) 2 (K sp = 3.9 *10 −6 ) are thrown into 3.00 L of water, solve for the concentration of Zn 2+ and IO 3 − . 12. Given a 1.00 L solution that is 0.100 M ZnNO 3 and 135 g of Zn(IO 3 ) 2 are added to the solution, what would be the concentration of Zn 2+ and IO 3 − . (Use K sp from previous question) 13. For a 1.00 L solution of 0.0250 M PbI 2 (K sp = 7.9 * 10 −9 ), would a precipitate be expected?...
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This note was uploaded on 11/30/2011 for the course CHEM 1212 taught by Professor Dockery during the Fall '08 term at Kennesaw.

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Test 3 Practice - NH 3 NO 3 K b(CH 3 NH 2 = 4.4 10 −6 Test 3 Practice 10 Classify the salt CH 3 NH 3 NO 2 as acidic basic or neutral(see question

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