Determine the pH you expect to find for the three solutions in question 2? Quest

Question

Determine the pH you expect to find for the three solutions in question 2? Question 2 states: a buffer solutions contains .120M acetic acid and 0.150 M sodium acetate. a) how many moles of acetic acid and of sodium acetate are present in 50.0 mL of solution= 0.0075 b) if we add 5.55 mL of 0.092 M NaOH to the solution in part a, how many moles of acetic acid, sodium acetate, and NaoH will be present after the reaction is done= 0.0055 acetic acid, 0.0005 NaOh, 0.008 sodium acetate C) if we add 0.50 ml of 0.087 M hcl to the solution in part a, how many moles of acetic acid ,sodium acetate and NaOH will be present after the reaction is done? = 0.006 acetic acid,.0075 sodium acetate PLEASE SHOW WORK

Explanation / Answer

HClO4 + H2O ----> ClO4- + H3O+
therefore, H+ concentration = concentration of HClO4.

HCl + H2O ----> Cl- + H3O+
therefore, H+ concentration = concentration of HCl.

oh, if both compounds are present in the same solution, you simply have to add up the concentrations of H+...

total [H+] = 5.8x10^-2 + 3.0x10^-2 = 0.088 M (to 6 significant figures.)

pH = -lg (0.088)
=1.06 (to 3 significant figures).

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