What is the concentration of [H^+] in molars, millimolars, and micromolars for a

Question

What is the concentration of [H^+] in molars, millimolars, and micromolars for a solution of pH 5? If you mix 10mL of a 0.1 M HCl solution with 8mL of a 0.2M NaOH solution, what will be the resulting pH? If a weak acid, HA, is 3% dissociated in a 0.25 M solution, calculate the K_a and the pH of the solution. What is the pH of a 0.05 M solution of TRIS acid (pK_a = 8.3)? What is the pH of a 0.045 M solution of TRIS base? If you mix 50mL of 0.1 M TRIS acid with 60mL of 0.2M TRIS base, what will be the resulting pH? If you add 1 mL of 1 M NaOH to the solution in 6 above, what will be the pH? How many total milliliters of 1 M NaOH can you add to the solution in Problem 6 and still have a good buffer (that is, within 1 pH unit of the pK_a)? If you are making 100mL of a 0.1 M HEPES buffer starting from HEPES in the basic form, is it prudent to get 50 mL of 1 M HCl from the community reagent bottle to use for your titration?

Explanation / Answer

Ans 3.

pH = -log [H+]

[H+] = 10-pH

=10-5

= 0.00001 M

or 0.01 millimoles

or 10 micromoles

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