a pH 222 b pH 505 c pH 700 d pH 106 9 What are the 7 strong acids 10 Which of

# A ph 222 b ph 505 c ph 700 d ph 106 9 what are the 7

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a)pH = 2.22 b)pH = 5.05c)pH = 7.00d)pH = 10.6 9. What are the 7 strong acids?10. Which of the following would be a stronger acid? A.HNO3vs. HNO2B.H2SO3vs H2FO311. Determine whether each of the following salts will form a solution that is acidic, basic, or neutral. A.SrCl2B.KI C.Cu(NO3)2D.NaClO
12.Write out the equilibrium-constant expressions for the following. What would the value of Kc be for part (a) if the reaction had been reverseda.CO(g) + H2O(l) H2(g) + CO2(g) Kc = 1.7 x 10-1b.Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g) c.SbCl5(g) SbCl3(g) + Cl2(g) 13.If we start the experiment with a mixture of 0.275 mole of NOBr(g), 0.185 mole of NO(g), and 0.075mole Br2(g) in a 0.500 L container at 100oC, would more NO(g) + Br2(g) be formed or consumed? 2NOBr(g) 2NO(g) + Br2(g)Kc = 0.01414.For the reaction 2SO3(g) 2SO2(g) + O2(g), Kc is 2.71 x 10-3at 925K. Write the equilibrium expression. Calculate the Kp value for this reaction at this temperature. 15.A closed system initially containing 1.750x10-3M H2and 2.750x10-3M I2at 448oC is allowed toreach equilibrium, and at equilibrium the HI concentration is 2.200x10-3M. Calculate the Kcat this temperature for the reaction H2(g)+I2(g)2HI(g)
16.Calculate the pH of a 0.155 M HCN solution. KaHCN = 3.5 x 10-4.

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