Write the balanced chemical equation for the following acid and base reaction. (use the lowest possible whole number coefficients. include states-of-matter under the given conditions in your answer.)
hbr(aq) + lioh(aq) →
a) using the balanced reaction above, calculate the amount of 0.0024 m lioh that would neutralize 22 ml of 0.0026 m hbr.
b)how many moles of salt are produced in the reaction?
c)what is the molar concentration of the salt after the reaction is complete?

Explanation:

a)Molarity of LiOH, = 0.0024 M

Volume of LiOH =

Molarity of HBr, = 0.0026 M

Volume of HBr =

According to reaction , 1 mol of LiOH neutralizes 1 mol of HBr.

Moles of LiOH =

Mass of 0.0571 mol of LiOH:

1.3704 g of 0.0024 M LiOH that would neutralize 22 mL of 0.0026 M HBr.

b) According to reaction , 1 mol LiOH gives 1 mol of LiBr.

Then ,0.0571 mol of LiOH will give:

of LiBr

0.0571 moles of salt are produced in the reaction

c) Moles of salt = 0.0571 mol

Volume of the solution = 22 ml+ 23.8333 mL= 45.8333 mL = 0.0458333 L

Molar concentration of the salt:

1.2458 mol/L is the molar concentration of the salt after the reaction is complete.

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