Chemistry

Find the [H3O+] in a solution having [OH-] = 8.8x10^-2 M

[H3O+]x[OH-]=1x10^-14
[H3O+]x[8.8x10^-2]=1x10^-14

i am almost sure i am right up to here but i don't know what to do next and i don't have a scientific calculator.. please help!!

  1. 👍 0
  2. 👎 0
  3. 👁 259
  1. Good lord. YOu will not pass Chemistry, nor learn it,without a scientific calculator. Just how do you plan on getting logarithms?

    PUt this in your google search window:

    1E-14 / 8.8E-2

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.9×10−9M Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 2.1×10−2M Calculate [H3O+] in the following aqueous solution at 25

    asked by Brandon on April 29, 2014
  2. chemistry

    1. Find the pH of a solution whose [H3O+] is 9.5 X 10^ -8 M. 2. What is the [H3O+] concentration of a solution with a pH of 5.45? 3. What is the pOH of a solution with a [OH -] concentration of 2.97 X 10^ -10 M?

    asked by kellin on May 14, 2012
  3. chemistry

    The weak acid HQ has pKa of 4.89. 1)Calculate the [H3O+] of .035 M HQ. 2)Calculate the (OH-) of 0.500 M HQ ....Am I correct? a) pKa = 4.89 => - log(Ka) = 4.89 => Ka = antilog(- 4.89) = 10-4.89 = 1.29x10-5 1. Given concentration of

    asked by patrick on October 4, 2015
  4. Chemistry

    Write a balanced equilibrium equation and kb expression for the reaction of the hydrogen phosphate ion (HPO4^2-) with water. Answer: HPO4^2-(aq) +H2O(l) PO4^3-(aq) +H3O+ (aq) kb= [PO4^3-][H3O+]/ [HPO4^2-] is that right?

    asked by Anonymous on May 13, 2012
  5. chemistry

    How many moles of H3O+ or OH- must you add per liter of HA solution to adjust its pH from 9.75 to 9.01? Assume a negligible volume change. ……….x 10………Moles of ……………………..h3O+ or OH- I got 4.6001 x 10-5 M

    asked by patrick on October 4, 2015
  1. chem

    Calculate the pH of 0.20 M NaCN solution. NaCN ---> Na+ + CN- CN- + H20+ ---> HCN+ + OH- Initial conc. of CN- = 0.20 mol/L change = -x equillibrium = 0.20-x HCN equill. = +x OH equill. = 1x10^-7+x Ka= 6.2 x 10^-10 Kb = KW/Ka =

    asked by Lena on July 24, 2009
  2. Math; PLEASE CHECK MY ANSWERS

    1.Which of the following is greater than 4.3x10^9 A)2.1x10^9 B)3.2x10^9 C)5.3x10^9 D)7.4x10^8*** 2.Which of the following are less than 6.5x10^-5? A)1.4x10^-3 B)2.5x10^-4 C)7.8x10^-5 D)4.6x10^-6*** 3.Which number is greater than

    asked by Anonymous on October 5, 2015
  3. chemistry

    AlPO4(s)Al^3+(aq)+PO4^3-(aq) PO4^3-(aq)+H3O^+(aq)HPO4^2-(aq)+H2O(l) What is the net ionic equation for AlPO4(s) dissolving in H3O^+(aq)?

    asked by CHEMistry on March 16, 2009
  4. Chemistry

    In the equilibrium system CH3COOH(aq) + H2O(l) —> — H3O+ CH3COO-(aq) .

    asked by L on January 21, 2018
  5. Chem

    CH3COOH(aq) + H2O(l) ⇌ H3O^+(aq) + CH3COO^–(aq) [H3O^+] = 4.0 × 10^–3 M [CH3COOH] = 0.90 M What is the Ka value for the reaction?

    asked by Summer on March 30, 2018
  6. chemistry

    Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products. HCHO2(aq)+H2O(l)⇌H3O+(aq)+CHO−2(aq) Use A for [HCHO2], B for [H2O], C for [H3O+], D for [CHO−2].

    asked by Anon on December 3, 2014

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