You dilute a solution of 0.100 mol of H3PO4 and 0.150 mol of NaOH with water to a volume of 1.00 L but then realize that the distilled water used was actually dilute hydrochloric acid.
For H3PO4: Ka1= 7.5 x 10^-3; Ka2= 6.2 x 10^-8; Ka3= 4.8 x 10^-13.
a) First calculate pH of the original solution. Write out a balanced equation for any neutralization reaction that occurs. (Hint: you do not actually need to find [H3O+] to calculate pH!)
b) If the actual pH of the solution (with added HCl) is 6.73, what are the concentrations of H3PO4, H2PO4-, and HPO4 2-? How many moles of HCl were mistakenly added to the original solution? Write out a balanced reaction for any neutralization reaction that occurs