Which of the following is the pH of a 0.0295 M NaOH solution-? 7.00 12.47 1.53 3

Question

Which of the following is the pH of a 0.0295 M NaOH solution-? 7.00 12.47 1.53 3.39 Times 10^-13 None of the above Which reaction will shift toward products when the volume of the reaction container is increased? N_2(g) + 3 H_2(g) rightarrow 2 NH_2(g) H_2(g) + I_2(g) rightarrow 2 HI_2(g) All of the above shift towards products None of the above shift towards products The following equilibrium reaction has a K, of 7.55 Times 10^-2 at 73 degrees C. What is the K.? SO_2(g) + O_2(g) rightarrow 2 SO_3(g) 691 691 1.17 Times 10^-5 8.248 Times 10^-4 2.66 Times 10^-3 All of the following are strong acids except HBr HCl HI HF They are all strong acids In an equilibrium constant expression: The pressures of pure liquids are included The concentrations of aqueous solutions arc included The concentrations of solids arc included All of the above None of the above

Explanation / Answer

11. pH of a 0.0295M NaoH solution

NaOH(aq) Na+(aq) + OH- (aq).

Therefore the concentration of OH- in the final solution is 0.0295 M. pOH = -log[OH-] = -log(0.0295) = 1.53

pKW = pH + pOH = 14.00 pH = 14.00 – 1.53 = 12.47

There fore answer is B.

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