chemistry

Calculate the pH after 0.15 mol of NaOH is added to 1.00 L of the solution that is 0.50 M HF and 1.01 M KF

  1. 👍 0
  2. 👎 0
  3. 👁 216
  1. Use the Henderson-Hasselbalch equation and set up an ICE chart for the NaOH and HF.

    1. 👍 0
    2. 👎 1

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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

  2. Chemistry

    Use the dilution relationship (Mi x Vi = Mf x Vf) to calculate the volume of 0.500 M NaOH needed to prepare 500 mL of .250 M NaOH. This is my work ? L Solution = 500mL x (1L/1000mL) = .500L ? mol NaOH = .500 L Solution x (0.250 M

  3. Grade 12 chemistry

    This is the second reaction: HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l) (Heat of neutralization) This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl. Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL

  4. Chemistry

    What is the molality of a glucose solution prepared by dissolving 18.0g of glucose, C6H12O6 in 125g of water? A)0.000794 B)0.144 C)0.699 D)0.794 Molality is the number of moles of solute per kilogram of solvent. Because the

  1. Chemistry

    500.0 mL of 0.220 mol/L HCl(aq) was added to a high quality insulated calorimeter containing 500.0mL of 0.200 mol/L NaOH(aq).Both solutions had a density of 1g/mL & a specific heat of 4.184 J/g.K.The calorimeter had a heat

  2. Chemistry

    How would you calculate the pH of the buffer if 1.0mL of 5.0M NaOH is added to 20.0mL of this buffer? Can someone please explain to me how to do B and C step by step so I could understand it clearly? :) Say, for example, that you

  3. Chemistry

    1.0L of aqueous solution in which [H2CO3]=[HCO3^-]=0.10M and has [H^+]=4.2E-7. What is the concentration of [H^+] ofter 0.005 mole of NaOH has been added? H2CO3 ==> H^+ + HCO3^- k1 = (H^+)(HCO3^-)/(H2CO3) I don't know if you are

  4. CHEMISTRY FOR DR. BOB or anyone else

    A hypothetical weak acid HA, was combined with NaOH in the following proportions: 0.20 mol HA, 0.08 mol NaOH. The mixture was then diluted to a total volume of 1L, and the pH measured. (a) If pH=4.80, what is the pKa of the acid

  1. chemistry

    Consider a solution containing 0.47 M HOCl and 0.67 M NaOCl for the next two questions. The Ka for HOCl = 3.5E-8. What is the pH of this solution? Now calculate the pH of this solution after 0.15 mol of NaOH is added to 1.00 L of

  2. Chemistry

    How would you calculate the pH of the buffer if 1.0mL of 5.0M NaOH is added to 20.0mL of this buffer? Can someone please explain to me how to do B and C step by step so I could understand it clearly? :) Say, for example, that you

  3. CHEM

    Which of the following mixtures will result in the formation of a buffer solution when dissolved in 1.00 L of water? i) 0.50 mol NaOH and 0.50 mol HCl. ii) 0.50 mol NaCl and 0.25 mol HCl. iii) 0.50 mol NaF and 0.25 mol HF. iv)

  4. Chemistry

    1)A solution prepared by adding 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate to 100.0 mL of water. The pH of this buffer solution is initially 4.74. Predict the final pH when 55.0 mL of 1.10 M NaOH is

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