Chemistry

Hydrogen cyanide is a weak acid with Ka = 4.9 x 10-10. Calculate the pH of a solution (to 2 decimal places) containing 2.28 g of Sr(CN)2 per 158 mL.

  1. 👍
  2. 👎
  3. 👁
  1. Sr(CN)2 ==> Sr+^2 + 2CN^-

    CN^- + HOH ==> HCN + OH^-

    Kb = Kw/Ka = (HCN)(OH^-)/(CN^-)

    Convert 2.28 g Sr(CN)2 per 0.158L to mols/L.(Note that Sr(CN)2 has 2 CN^- per mole of Sr(CN)2.)
    Plug x for (HCN) and x for (OH^-), solve for (OH^-), convert to pOH, then to pH.
    Post your work if you get stuck.

    1. 👍
    2. 👎
  2. Above posted by DrBob222.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem- REALLY URGENT!!!

    2. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the

  2. 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

  3. chemistry

    The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.

  4. AP Chemistry

    A 0.00100 M solution of a weak acid HX is 6% ionized. Calculate Ka for the acid.

  1. Please help me!!!!

    2. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the

  2. Chemistry

    Butyric acid (HC4H7O2) is a weak acid with the stench of rancid butter 1.) write the equation for the dissociation of HC4H7O2 in water 2.)the pH of .5 M HC4H7O2 is 2.56 calculate Ka of butyric acid 3.) Write the equation for the

  3. Chemistry-Dr Bob help!!

    0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid

  4. Chem Help please!!!!!

    2. Methane (CH4), ammonia (NH3), and oxygen (O2) can react to form hydrogen cyanide (HCN) and water according to this equation: CH4 + NH3 + O2  HCN + H2O You have 8 g of methane and 10 g of ammonia in excess oxygen. Answer the

  1. chemistry

    In a .25 M solution, a weak acid is 3.0% dissociated. A. calculate the pH of the solution B. calculate the Ka of the acid Please explain steps.

  2. Chemistry

    Which of the following aqueous solutions are good buffer systems ? . 0.26 M hydrochloric acid + 0.24 M potassium chloride . 0.14 M acetic acid + 0.20 M potassium acetate . 0.16 M potassium hypochlorite + 0.23 M hypochlorous acid .

  3. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?

  4. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?

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