College Chemistry

Calculate pH of a 1.0 mol L -1 boric acid solution.
(Ka(H3BO3) = 5.8 x 10 power -10

Please solve this problem. My computer does not have the power symbol.

Can you please show maths and steps.
Is mollar mass required of the above.
Is -log and constant above used.


  1. 👍
  2. 👎
  3. 👁
  1. H3BO3 ==> H^+ + H2BO3^-

    Set up an ICE chart, substitute into Ka expression, and solve for H^+. Then use pH = -log(H^+) to convert to pH.
    At equilibrium, you should have this substituted into Ka.
    5.8 x 10^-10=(H^+)(H2BO3^-)/(H3BO3)
    5.8 x 10^-10 = (x)(x)/(1-x)
    Solve for x, which is H^+, then convert to pH.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    The density of 19.0% by mass of nitric acid, HNO3 is 1.11 g cm-3. Calculate the volume (dm3) of acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution. (FW HNO3 = 63 g/mol)

  2. math 101

    how much liquid containing 6% boric acid should be mixed with 2 quarts of a liquid that is 15% boric acid in order to obtain a solution that is 12% boric acid?

  3. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka

  4. Chemistry

    (a) Calculate the molarity of a solution that contains 0.175 mol ZnCl2 in exactly 150 mL of solution. (b) How many moles of HCl are present in 35.0 mL of a 4.50 M solution of nitric acid? (c) How many milliliters of 6.00 MNaOH

  1. Chemistry

    1. What is the pH of a 1.0 x 10-3 M solution of boric acid, H3BO3? The Ka value for boric acid is 6 x 10-10. (choices: 3, 7, between 7 and 12, between 3 and 7) 2. You want to use a 0.500 M HNO3 solution to titrate an unknown

  2. Chemistry

    Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL

  3. chemistry

    25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L acetic acid. Calculate the pH of the solution

  4. Chemistry

    1. A lab tech needs 1.00 L of 0.125 mol/L sulfuric acid solution for a quantitative analysis experiment. A commercial 5.00 mol/L sulfuric acid solution is available from a chemical supply company. Write out what steps he/she would

  1. chemistry

    24 mL of 0.39 mol/L acetic acid is titrated with a standardized 0.33 mol/L KOH solution. Calculate the pH of the solution after 17 mL of the KOH solution has been added. Assume the Ka of acetic acid is 1.8 x 10-5.

  2. Chemistry - Buffers

    A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer? A. .01 mol B. .05 mol C.

  3. chemistry

    Lactic acid, HC3H5O3(aq) is a weak acid that gives yougurt its sour taste(Yeeeeecccckkk). Calculate the pH of a 0.0010 mol/L solution of Lactic acid. The Ka for lactic acid is 1.4 x 10^-4


    A 1.575 g sample of ethanedioic acid crystals, H2C2O4. xH20 was dissolved in water and made up to 250cm^3 . One mole of the acid reacts with two moles of NaOH. In a titration, 25.0 cm^3 of this solution of acid reacted with

You can view more similar questions or ask a new question.