QUESTION 2 2.1.1 What is the total molar concentration of ions in each of the following solutions: A 1.250 M solution of CH₂OH. 2.1.2 A solution of HCI in water conducts electricity but a solution of of HCI in chloroform does not. What does this observation tell you about the way HCI exists in water and the way it exists in chloroform? 2.2 Classify each of the following reactions as precipitation, acid base neutralization or oxidation-reduction: 2.2.1 2CH3CO₂H (aq) + Ba(OH)2 (aq) → (CH3CO₂)2Ba (aq) + 2H₂O(l) 2.2.2 NiCl₂ (aq) + Na₂S (aq) → NiS (s) + 2 NaCl (aq) 2.2.3 Hg(NO3)2(aq) + 2 Nal(aq) → 2 NaNO3(aq) + Hgla(s)

QUESTION 2 2.1.1 What is the total molar concentration of ions in each of the following solutions: A 1.250 M solution of CH₂OH. 2.1.2 A solution of HCI in water conducts electricity but a solution of of HCI in chloroform does not. What does this observation tell you about the way HCI exists in water and the way it exists in chloroform? 2.2 Classify each of the following reactions as precipitation, acid base neutralization or oxidation-reduction: 2.2.1 2CH3CO₂H (aq) + Ba(OH)2 (aq) → (CH3CO₂)2Ba (aq) + 2H₂O(l) 2.2.2 NiCl₂ (aq) + Na₂S (aq) → NiS (s) + 2 NaCl (aq) 2.2.3 Hg(NO3)2(aq) + 2 Nal(aq) → 2 NaNO3(aq) + Hgla(s)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 106CP

See similar textbooks

Similar questions

A 0.0515 g pure potassium dichromate was dissolved in water and a large excess of KI was added. The liberated iodine required 45.54 mL of thiosulfate solution. Calculate the molarity of Na2S2O3. Choices: 0.384 M, 0.0231 M, 0.00200 M, 1.050 M
The balanced net ionic equation for the neutralization reaction involving equal molar amounts ofHCl and CH3CH2NH2 is ________.
To prepare a stock solution of EDTA, 73 grams of EDTA were mixed to 500 mL of distilled water. What is the: A. Molar concentration of EDTA stock solution is Blank 1M Using the prepared EDTA stock solution above, 25 mL of 200 mM working solution has to be made. Calculate for the following: B. Volume of EDTA stock solution to be diluted is Blank 2mL C. Volume of distilled water is Blank 3mL
State the chemical name of Plaster of Paris. Write a chemical equation to show the reaction between Plaster of Paris and water
Balance the following in acidic medium: MnO4- + Fe2+ ---> Mn2+ + Fe3+ How many Fe2+ are there in the balanced equation?
An unknown metal M forms a soluble compound,M(NO3)2.A solution of M(NO3)2 is electrolyzed. When a constantcurrent of 2.50 amperes is applied for 35.0 minutes,3.06 grams of the metal M is deposited.1.1 Calculate the molar mass of M and identify themetal.
Clorox is a laundry bleaching agent used to remove stains from white clothes. Suggest why the name begins with Clor- and ends with -ox. Group of answer choices Chlor- because it has chlorine ions, -ox because it uses oxygen. The active ingredient contains chlorine atoms, which behave as strong oxidizing agents. Chlor- because it has chlorine ions, -ox because it is reduced. Clor- because it has chlorine, -ox because it is as strong as an ox.
Provide a step-by-step solution to the problem.
How many grams of calcium phosphate can be produced from the reaction of 2.75 L of 0.650 M Calcium chloridewith and excess of phosphoric acid? Write the balanced equation and the complete solution. Please answer immediately i need it for 5 mins
21, 33
What is the normality and molarity of a solution of KMnO4 if 40.00 ml will oxidize 0.3000g of FeSO4.7H2O? Note: Please present complete solution. If you answered it already, please skip this. I'm posting it again to compare the answers thanks!
An impure sample H2C2O4 was oxidized by KMnO4. A 0.262g sample of H2C2O4 was dissolved, and the solution was diluted to 100mL. A 25mL portion of H2C2O4 solution was titrated with 25.2mL of 0.0107M KMnO4. What is the balanced equation for the titration reaction and how many moles of KMnO4 were used?