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When zinc metal is reacted with hydrochloric acid, zinc chloride and hydrogen gas are produced. If 16.4 ml of 2.14 M HCl are used:

a) how many grams of zinc metal are needed to completely use up the acid?

b) What will be the molarity of the aqueous product?

Please show all work. Thank you!

  • chemistry -

    I wont show all work, ever. What teacher would ever do that?

    balance the equation
    Zn+ 2HCl>>ZnCl2 (aq) + H2(g)
    so for each mole of acid, you need half that moles of Zn.

    moles HCL: Volume*concentraioninMolarity
    moles of Zn needed: half of that.
    grams of Zn: molesZn*atomicmassZn
    Molarity of product? it is a solution of ZincChloride: figure the moles of ZnCl2 made (same moles as Zn), then
    molarityZnCl2= molesZnCl2/volume
    where volume is still .0164 liters.

  • chemistry -

    This is a regular stoichiometry problem.
    Zn + 2HCl ==> ZnCl2 + H2

    1. Convert HCl to moles. moles = M x L = ?
    2. Use the coefficients in the balanced equation to convert moles HCl to moles Zn.
    3. Convert moles Zn to grams. g = moles to molar mass.

    b) Convert moles (either Zn or HCl) to moles ZnCl2. Then M = moles/L.

  • chemistry -

    Thank you both for your help! You made it very clear

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