posted by .

If 100mL of a 0.10M NaOH solution is added to 75mL of a 0.15 HCl solution, then what is the pH of the resultant solution?

  • Chemistry -

    Write the equation.
    HCl + NaOH ==> NaCl + H2O

    mols NaOH = M*L = 0.10 M x 0.1 L = ??

    mols HCl = M*L = 0.15 M x 0.075 L = ??

    See which is in excess, how much is left over after reacting, then pH = - log(H^+). Post your work if you get stuck.

  • Chemistry -

    I don't understand where the H+ comes from, I mean I know it comes from the acid, but don't I need an equilibrium constant K to solve for the H+?

  • Chemistry -

    No. Since the product is NaCl and water and the NaCl doesn't hydrolyze, the H+ or OH- comes from the excess of HCl OR NaOH. Look at the mols HCl and the mols NaOH. Calculate each according to my last post. You will see one is larger than the other. So subtract them to find the difference and that will be the H+ if it is the HCl in excess OR it will be the OH- if it is the NaOH in excess. Both HCl AND NaOH are strong acids and bases so neither has a Ka or Kb.

  • Chemistry -

    A note that when you subtract the difference is the MOLS of excess reagent. The concentration is mols/L to calculate H+ or OH- so mols/0.175 L is the concentration.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Math

    What volume, in ml, of a 60% of HCl acid solution must be added to 100 ml of a 30% HCl solution to make a 36% HCl solution. We need 2 alegabreic (?
  2. AP Chemistry

    A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with …
  3. Chemistry

    I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems?
  4. chemistry

    100ml solution made up 1.0M NH3 and (NH4)2SO4 have been added with 100ml of 0.1 HCl. how many moles are present in the solution before and after?
  5. High School Chemistry

    10mL of 0.10M HCl is given. What is the pH?
  6. chemistry

    Draw the tritration curve for the neutralization of a 100ml sample of 1M solution of HCl with a .6M solution of Naoh point 1: 2 ml NaOH edded point 2: 40 ml NoOH ADDED POINT 3: EQUIVALENCE POINT 4: 80 ML NaOH added
  7. Chemistry

    a solution is made by combining 10.0 ml of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. a)calculate the pH of the solution. b) how many grams and milliliters of 14.6 M potassium hydroxide …
  8. chemistry

    1)100ml sample of solution that is 0.2m in both Naf and Hf has 4.0 ml of 1.0m hcl added to it. calculate the ph change of this soultion .ka =7.2*10^-4 2)40 ml of 0.32m benzoic acid if titrated with 60 ml of 0.2 m naoh. clacilate the …
  9. Chemistry

    A solution is prepared by dissolving of pure HC2H3O2 and of NaC2H3O2 in of solution (the final volume). (a) What is the pH of the solution?
  10. chemistry

    A student prepares a solution of hydrochloric acid that is approximately 0.1 M and wanted to determine its precise concentration. A 25.00 mL portion of the HCl solution is transferred to a flask, and after a few drops of indicator …

More Similar Questions