Chem 20

posted by .

Calculate the mass of strontium hydroxide required to make a 450-mL solution with a pOH of 4.00.

Step 1: Find pOH. I found that pOH is 10.

The next steps is where I'm stuck.

Step 2 :Calculate the hydroxide ion concentration. Express your answer in scientific notation.
Spell check
mol/L.
Answer:
Step 3: Calculate the concentration of strontium hydroxide. Express your answer in scientific notation.
Spell check
mol/L.
Answer:

Step 4: Determine the number of moles of Sr(OH)2(aq). Express your answer in scientific notation.
Spell check
mol.
Answer:

Step 5: Determine the mass of Sr(OH)2(s)

  • Chem 20 -

    The pOH is 10.
    To convert pOH = 10 to OH^-, it is
    pOH = -log(OH^-)
    10 = -log(OH^-)
    -10 = log(OH^-)
    Take antilog of both sides.
    1 x 10^-10 = OH^-

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chem

    hey guys I posted this awhile ago im not sure if anyone has read it or whatever but here it is again find the PH of a .00580 M solution of the strong base KOH. is it -log(.00580)= 2.24 pOH = -log[OH-] pH + pOH = 14.00 Therefore, pOH …
  2. chem

    this is my question Calculate the hydronium ion consentration and the hydroxide concentration in blood in which the PH is 7.3. I don't have invlog on my calculator so I hit log(7.3)= .863 for hydronium. Is this dumb for me to do?
  3. chemistry

    What mass in grams of potassium hydroxide is contained in 500 mL of solution that has a pH of 11.5?
  4. Physical Chem

    A student added solid K2O to a 750.0 mL volumetric flask. The solid was dissolved in water and then the flask filled with water to the mark. This formed 750.0 mL of the initial KOH solution. 20.0 mL of the initial solution was transferred …
  5. Chemistry

    Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=?
  6. Chemistry

    Each value below represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. pH=9.72 pOH=4.69 pOH=13.62 [H+]=7.5e-2 [H+]=7.8e-9 [H+]=1e-7 [OH-]=4.5e-12 [OH-]=3.5e-5 pH=4.09 pOH=7
  7. Chemistry

    Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=?
  8. Chemistry

    Sometimes the basicity of a solution is reported using pOH (pOH = -log[OH-]). What is the a. [OH-] if pOH = 1.90 b. [H3O+] if pOH = 12.94 c. pH if pOH = 9.70
  9. chemistry

    Sometimes the basicity of a solution is reported using pOH (pOH = -log[OH-]). What is the a. [OH-] if pOH = 1.90 b. [H3O+] if pOH = 12.94 c. pH if pOH = 9.70
  10. Chemistry

    My school notes say : pH < pOH is acidic pH > pOH is basic Is this correct, I was thinking that if the pH is less than pOH than it was a basic solution

More Similar Questions