Another chemistry student in a different laboratory titrated 18.0 mL of unknown H2SO4 (aq) solution with 38.2 mL of 0.163 M KOH to its final endpoint. What is the unknown molarity concentration of the sulfuric acid solution that went through the acid/base neutralization reaction shown below? 1 H2SO4 (aq) + 2 KOH (aq) --> K2SO4 (aq) + 2 H2O (l)

A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH(aq) →A¯(aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 10 ", is titrated with NaOH. 6 Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit ▾ Part B pH = IVE] ΑΣΦ Submit A → c More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 66.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IVE ΑΣΦ A + Ċ ? Doowoon Review | Constants | Periodic Table ?

The standardized NaOH was used to determine the unknown concentration of H3PO4. The standard NaOH concentrtion is 0.126M. The standard sulfuric acid concentration is 0.150M. 3 NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3 H2O(l) Three flasks containing 25.00 mL H3PO4 each was titrated with NaOH. The data is below:                                    Titration 1       Titration 2.           Titration 3 Starting volume buret 2.62 mL           18.60 mL            1.20mL Buret volume at end 18.46 mL            34.40mL             16.84mL Calculate the concentration of H3PO4.

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.