When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following is correct for this titration: Initially the pH will be less than 1.00. The pH at the equivalence point will be 7.00. It will require 12.50 mL of NaOH to reach the equivalence point. View Available Hint(s) When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following is correct for this titration: Initially the pH will be less than 1.00. The pH at the equivalence point will be 7.00. It will require 12.50 mL of NaOH to reach the equivalence point. B and C only B only A and B only A and C only

The correct options are B and C only

Explanation:

The equivalence point of a chemical reaction is the point at which chemically equivalent quantities of reactants have been mixed to form products. For an acid-base titration or neutralization reaction, the equivalence point is the point at which equal moles of acid and the moles of base that would neutralize each other according to the chemical reaction has been mixed.

The reaction in which 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr is a neutralization reaction and at equivalence point, pH = 7.00. The equation of the reaction is given below:

HBr + NaOH > NaBr + H₂O

Using the formula: CaVa/CbVb = Na/Nb

Where Ca = concentration of acid; Va = volume of acid; Cb= concentration of base; Vb = volume of base; Na/Nb = mole ratio of acid and base

Ca = 0.050 M

Va = 25.00 mL

Cb = 0.100 M

Vb = ?

Na/Nb = 1

Vb = CaVa/Cb * 1

Vb = (0.050 * 25 mL/ 0.100) * 1

Vb = 12.50 mL

Therefore, 12.5 mL of  0.100 M NaOH is required to neutralize 25.00 mL of 0.0500 M HBr

The correct options are B and C only