HW_1 - 7. Write the equilibrium constant expression for...

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CHEM 150 HOMEWORK #1 Due: Thursday, 4/5/10 1. How many grams are contained in 450. mL of 0.250 M methanol (CH 3 OH)? 2. A solution was prepared by dissolving 432 mg of K 4 Fe(CN) 6 in water and diluting to 1.5 L. Calculate the K + concentration in ppm. 3. Any dilute aqueous solution has a density near 1.00 g/mL. If a given solution is 1.0 ppm solute, determine the concentration of solute in ȝ g/L. 4. What is the density of 53.4 wt% aqueous NaOH if 16.7 mL of the solution diluted to 2.00 L gives 0.169 M NaOH? 5. How many milliliters of 3.00 M H 2 SO 4 are required to react with 4.35 g of solid containing 23.2 wt% Ba(NO 3 ) 2 if the net ionic reaction is: Ba 2+ + SO 4 2- ĺ BaSO 4 (s). 6. Write each answer with the correct number of significant figures. log(4.128x10 12 ) = ? 10 2.384 = ? e -10.45 = ? 5.45/antilog(-3.22) = ?
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Unformatted text preview: 7. Write the equilibrium constant expression for 2CrO 4 2-+ 2H + = Cr 2 O 7 2-+ H 2 O 8. Calculate the molar solubility of silver bromide (K sp = 5.2 x 10-13 ) in 0.0250 M KBr. 9. Hydrocarbons in the cab of an automobile were measured during trips on the New Jersey Turnpike and trips through the Lincoln Tunnel connecting New Jersey and Manhattan. The total concentrations ( standard deviations) of m- and p-xylene were: Turnpike: 31.4 30.0 g/m 3 (32 measurements) Tunnel: 52.9 29.8 g/m 3 (32 measurements) Determine the 95% confidence interval for each experiment? Does the level of xylene differ in the two tunnels at 95% confidence? Justify your answer. 10. Calculate the pH of 0.010 M HCl, 0.035 M KOH, 0.030 M HNO 3 and 3.0 M HCl....
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This note was uploaded on 10/19/2010 for the course CHEMISTRY Chem150 taught by Professor De vries during the Fall '10 term at UCSB.

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HW_1 - 7. Write the equilibrium constant expression for...

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