Calculate the molarity of an acetic acid solution if 56.85 mL of the solution is needed to neutralize 164 mL of 1.03 Msodium hydroxide. The equation for the reaction is HC 2H 3O 2( aq)     +     NaOH( aq)     ---->     Na +( aq)     +    C 2H 3O 2 -( aq)     +     H 2O( aq)

If 55.0 mL of a 0.25M solution of Mg(OH)2 is spilt on the floor, what volume, in mL, of 0.15M HBr  is needed to neutralize the base?  2HBr(aq) + Mg(OH)2 --> 2H2O(l) + MgBr2(aq)

For the following acid-base neutralization: 2 HNO3 (aq) + Ca(OH)2 (aq) --> 2 H2O (I) + Ca(NO3)2 (aq) determine the volume (in mL) of 0.250 M calcium hydroxide solution needed to neutralize 16.1 ml of 1.35 M nitric acid solution.

A CHEM 1151K student notices that it takes 20.0 mL of a 1.5 M solution of KOH to completely neutralize 25.0 mL of carbonic acid (H2CO3). What is the molarity of the acid?H2CO3 (aq)   + 2KOH (aq)   ----->      Na2CO3 (aq)   +   2H2O  (l) 0.80 M H2CO3 0.40 M H2CO3 1.8 M H2CO 0.60 M H2CO3

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 ))

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.

What is the net ionic reaction for the titration of hydrobromic acid with sodium hydroxide? Group of answer choices OH−(aq) + HBr(aq) → Br−(aq) + H2O(l) OH−(aq) + H+(aq) → H2O(l) NaOH(aq) + HBr(aq) → NaBr(aq) + H2O(l) NaOH(aq) + H+(aq) → H2O(l) + Na+(aq)

Calculate the number of milliliters (mL) of a 0.125 M solution of KOH will be required to titrate 40.0 mL of a 0.0665 M solution of H3PO4. The equation for the reaction is H3PO4(aq)  +  2KOH(aq)  →  K2HPO4(aq)  +  2H2O(l).

25.0 mL of a Ba(OH)2 solution are titrated with hydrochloric acid. If 12.10 mL of 0.0825 M HCl are needed to reach the endpoint of the titration, what is the molarity of the Ba(OH)2 solution? HCl (aq) + Ba(ОН)2 (аq)