Answer:
1.31 M
Explanation:
Step 1:
Data obtained from the question. This include the following:
Volume of Base (Vb) = 0.080L
Molarity of base (Mb) =..?
Volume of acid (Va) = 0.0293L
Molarity of acid (Ma) = 3.58 M
Step 2:
The balanced equation for the reaction. This is given below:
H2CrO4 + Ca(OH)2 → CaCrO4 + 2H2O
From the balanced equation above,
The mole ratio of the acid (nA) = 1
The mole ratio of the base (nB) = 1
Step 3:
Determination of the concentration of base.
The concentration of the base can be obtained as follow:
MaVa/MbVb = nA/nB
3.58 x 0.0293 / Mb x 0.080 = 1
Cross multiply
Mb x 0.080 = 3. 58 x 0.0293
Divide both side by 0.080
Mb = (3.58 x 0.0293)/0.08
Mb = 1.31 M
Therefore, the concentration of the base, Ca(OH)2 is 1.31 M
