H,PO4 is both a weak acid and a weak base

A 50.0 mL sample of H2SO4 is neutralized with a KOH solution having a concentration of 0.400 M. If 22.6 mL of KOH are required to complete the neutralization, what is the concentration of the sulfuric acid solution?

Write the net ionic equation for the acid‑base reaction. Include physical states.   HCl(aq)+LiOH(aq)⟶H2O(l)+LiCl(aq)

What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by diluting 20.0 mL of concentrated (11.6 M ) HCl to a final volume of 500.0 mL?

A 50.00 mL sample of a locally made white wine required 34.50 mL of 0.0450 M NaOH to reach the end point. Express the acidity of the wine in grams of tartaric acid (H­2C4H4O6)

None

Complete and balance the following acid-base neutralization reactions: 1) HClO4 + NaOH (perchloric acid and sodium hydroxide) 2) H2SO4+ Ca(OH)2 (sulfuric acid and calcium hydroxide) 3) HC2H3O2 + NaOH (acetic acid and sodium hydroxide) 2) H2SO4+ Ca(OH)2 (sulfuric acid and calcium hydroxide) 3) HC2H3O2 + NaOH (acetic acid and sodium hydroxide)

What is the net ionic equation for the neutralization of hydrofluoric acid (HF) with sodium hydroxide? (Hint: it is NOT H(aq) + OH (aq) H(aq) + OH(aq) -> H₂O ))

HNO3(aq) + HCl(aq) = 1. what is the balanced equation 2. what is the ionic equation 3. what is the net ionic equation

Phosphoric acid (H3PO4) is a triprotic acid with three ionizable protons. Write a balanced equation for the neutralization of phosphoric acid with NaOH. How many milliliters of 0.250 M NaOH would be required to completely neutralize 40.0 ml of 0.080 M H3PO4?