What is the pH of a solution that is 0.21 M sodium fluoride and 0.57 M hydrofluoric acid?

From the Henderson- Hasselbalch equation, the pH of a solution is 3.36.How can the pH of a solution made from a weak acid and its conjugate base be calculated?The pH of a solution made from a weak acid and its conjugate base can be calculated using the Henderson- Hasselbalch equation.The Henderson- Hasselbalch equation is given below as follows:pH = pKₐ + log ([A⁻]/[HA])where;pKa = - log(Ka) of hydrofluoric acid[A⁻] = concentration of salt of conjugate base, NaF[HA] = concentration of hydrofluoric acidpKa of HF = 3.8[A⁻] = 0.21 M[HA] = 0.57 MpH = 3.8 + log (0.21/0.57)pH = 3.36Learn more about Henderson- Hasselbalch equation at: https://brainly.com/question/13423434#SPJ1