If 11.00 mL of a standard 0.2831 M NaOH solution is required to neutralize 26.86 mL of H2SO4, what is the molarity of the acid solution?

0.1159 M

Explanation:

Using the formula below:

CaVa = CbVb

Where;

Ca = concentration/molarity of acid (M)

Cb = concentration/molarity of base (M)

Va = Volume of acid (mL)

Vb = volume of base (mL)

According to this question, the following information were given:

Ca = ?

Cb = 0.2831 M

Va = 26.86 mL

Vb = 11.00 mL

Using CaVa = CbVb

Ca × 26.86 = 0.2831 × 11

26.86Ca = 3.1141

Ca = 3.1141 ÷ 26.86

Ca = 0.1159

The molarity of the acid (H2SO4) solution is 0.1159 M

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

increased stability in the completion of fluorine's outer shell.