Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO₂. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? OH(aq) + HCHO, (aq) → CHO2 (aq) + H2O() NaOH(aq) + HCHO₂ (aq) NaCHO₂ (aq) + H₂O(1) OH(aq) + H3O+ (aq) → 2H₂O(1) NaOH(aq) + H3O+ (aq) → Na (aq) + 2H₂O(1)

Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO₂. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? OH(aq) + HCHO, (aq) → CHO2 (aq) + H2O() NaOH(aq) + HCHO₂ (aq) NaCHO₂ (aq) + H₂O(1) OH(aq) + H3O+ (aq) → 2H₂O(1) NaOH(aq) + H3O+ (aq) → Na (aq) + 2H₂O(1)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 46QAP: Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to...

See similar textbooks

Similar questions

A buffer solution made from hydrocyanic acid and potassium cyanide titrated with hydrochloric acid. What is the net ionic equation for the reaction ? a) H 3 O^ + (aq)+HCN(aq)=>H 2 O(l)+H 2 CN(aq) b) HCl(aq)+CN-(aq)=>HCN(aq)+C(-(aq); c) HCl(aq)+OH^ - (aq)=>H 2 O(l)+Cl^ - (aq) d)No answer text provided e) . H 3 O^ + (aq)+CN^ - (aq)=>HCN(aq)+H 2 O(l)
In the following acid-base titration experiment CH3COOH (aq) + NaOH (aq) ———-> CH3COONa (aq) + H2O (l). What is the molarity of the NaOH solution if 11.6 mL of 3.0 M acetic acid is required to neutralize the sodium hydroxide in 25.00 mL of NaOH solution? (a) 0.65 M (b) 6.5 M (c) 96.6 M (d) 1.392 M
Adding acid to the buffer, NH3-NH4*, will produce this (net ionic) reaction: H*(aq) +OH(aq)=H₂O(1) H*(aq)+NH4*(aq) NH3(aq)+H₂(g) O H*(aq) + NH4+ (aq)=NH5²+ (aq) O H*(aq)+NH3(aq)=NH4+ (aq)
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)
Using the following reaction, H2SO4 (aq) + 2 NaOH (aq) Na2SO4 (aq) + 2 H2O (l) calculate the molarity of the H2SO4 solution if 14.92 mL of NaOH was necessary to reach the endpoint of a titration. The molarity of the NaOH solution was 0.83 M and 25.18 mL of H2SO4 was added to the Erlenmeyer flask.
If 27.75 mLmL of 0.349 M HClM HCl is used to titrate 10.0 mLmL of aqueous ammonia to a methyl red endpoint, what is the molarity of the ammonia? When we write aqueous ammonia as NH4OH, the balanced equation is HCl(aq) + NH4OH(aq) → NH4Cl(aq) + H2O(l)
If 26.7 mL of 0.205 M KOH is required to completely neutralize 20.0 mL of a HC2H3O2 solution, what is the molarity of the acetic acid solution HC2H3O2(aq) + KOH(aq) →→ KC2H3O2(aq) + H2O(l)
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 50.mL of a 0.027M 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.
An unkown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with NaOH. The appropriate reactions are as follows: Citric acid: H3C6H5O7 (aq) + 3 NaOH (aq) --> 3 H2O (l) + Na3C6H5O7 (aq) Tartaric acid: H2C4H4O6 (aq) + 2 NaOH (aq) --> 2 H2O (l) + Na2C4H4O6 (aq) A 0.956 g sample requires 29.1 ml of 0.513 M NaOH for titration to the equivalence point. What is the unknown acid?
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)⟶CO2(g)+H2O(l)+CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 25.0 mL of a solution that is 0.200 M in HCl, how many grams of CO2 gas are produced?
Write a balanced net-ionic equation for the neutralization reaction between CH3COOH (aq) and Ba(OH)2 (aq). 2 CH3COOH (aq) + Ba(OH)2 (aq) --> 2 CH3COO- (aq) + 2 H₂O (1) + Ba²+ (aq) 2 CH3COOH (aq) + 2 OH" (aq) --> 2 CH3COO(aq) + 2 H₂O (1) CH3COOH (aq) + OH" (aq) --> CH3COO (aq) + H₂0 (1) OH(aq) + OH- (aq) --> H₂O (1) 2 H (aq) + 2 OH- (aq) --> 2 H₂O (1)
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 150.mL of a 0.053 M 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.