chemistry

in the lab there is a spill of 47.5mL of .500 mol/L Al(OH)3. How many grams of H2SO4 would be needed to neutralize the spill.

  1. 👍
  2. 👎
  3. 👁
  1. Write the equation.
    2Al(OH)3 + 3H2SO4 ==>Al2(SO4)3 + 6H2O

    moles Al(OH)3 = M x L = 0.500 x 0.0475 = ??

    Using the coefficients in the balanced equation, convert moles Al(OH)3 to moles H2SO4.
    ??moles Al(OH)3 x [3 moles H2SO4/2 moles Al(OH)3] = xx moles H2SO4.

    Convert moles H2SO4 to grams H2SO4. g = moles x molar mass

    [Note: Al(OH)3 is NOT a strong base, it isn't very soluble in water, and it is not corrosive. Neutralizing it with H2SO4 (a strong acid and VERY corrosive) is an extremely poor idea. I'm sure this was just a problem example but in practice it wouldn't be done.]

    1. 👍
    2. 👎
  2. so moles Al(OH)3 = M x L = 0.500 x 0.0475 = ??

    is 0.02375?

    1. 👍
    2. 👎
  3. yes

    1. 👍
    2. 👎
  4. okay so i got,

    0.02375 molAl(OH)3x3molH2SO4/2molAl(OH)3=0.035625molH2SO4

    0.035625molH2SO4x98.08g/molH2SO4= 3.4941g H2SO4 Correct? so the 3.4941g would be how much H2SO4 needed to neutralize the spill?

    1. 👍
    2. 👎
  5. yes. However, since you are limited to 3 significant figures (from the 0.500 and 47.5 mL) I would round that to 3.49 g.

    1. 👍
    2. 👎
  6. thanks!

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Honors Chemistry

    "How many grams of NH3 can be produced from the reaction of 28 g of N2 and 25 g of H2? N2 + 3H2 ---> 2NH3 ==> 28 g N2 x (1 mol N2/14.0 g N2) x (2 mol NH3/1 mol N2) x ( 17.0 g NH3/ 1 mol NH3) = 68 g NH3 25 g H2 x ( 1mol H2/2.0 g

  2. Chemistry

    1)The chemical formula for aspirin is C9H8O4. What is the mass of 0.40 mol of aspirin? How would I find this? 2)The gram molecular mass of oxygen is 16.0 g right? 3)How would I find the mass, in grams, of 3.01 x 10^23 molecules of

  3. Chemistry

    How many grams of sodium nitrate, NaNO3 are needed to make 250 ml of .500 M solution? MM of NaNO3 is 85 g/mol?? I'm not sure which equation to use, help please?

  4. chemistry

    If 15.0 grams of C3H6, 10.0 grams of oxygen, and 5.00 grams of NH3 are reacted, what mass of acrylonitrile can be produced assuming 100% yield, what mass of the excess reactants remain? 15g C3H6 (1 mol / 42.08 g) = .35 mol C3H6

  1. chemistry

    Find the mass in grams. a. 4.30 x 10^16 atoms He, 4.00 g/mol b. 5.710 x 10^23 molecules CH4, 16.05 g/mol c. 3.012 x 10^24 ions Ca^2+, 40.08 g/mol

  2. chemistry

    3CuCl2 *2H2O + 2Al = 3Cu + 2AlCl3 + 6H2O Determine the number of grams that should have been produced when 1.25g of copper (2) chloride dehydrate reacts with excess aluminum so i'm not really sure how you're supposed to calculate

  3. chemistry, plz check work

    NH3+H2S-->NH4HS

  4. Chemistry

    (1)Make 500 ML of 4N H3PO4. How many grams will be needed? (2) In a titration procedure, 20mL of 2N solution were required to titrate 5mL of an unknown solution. What is the normality of the solution? (3) How much of a 0.01M can

  1. 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

  2. chemistry

    If 0.500 mol NaN3 react, what mass in grams of nitrogen would result?

  3. chemistry

    a mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 2.00-L stainless-steel flask at 430C. Calculate the concentrations of H2, I2, and HI at equilibrium

  4. chemistry

    What mass in grams of potassium hydroxide is contained in 500 mL of solution that has a pH of 11.5? I have a pOH of 2.5 to get [OH] I do 10^-2.5 to get 0.001581138 Then I divide this by 2 to find the mols in 500 mL Then, grams =

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