Question

3. Which solution has the highest boiling point: 1.0 M CH3CH2OH or 1.0 M NaBr? Justify...

3. Which solution has the highest boiling point: 1.0 M CH3CH2OH or 1.0 M NaBr? Justify your answer and explain how this relates to vapor pressure.

12. For the reaction: H2 (g) + Br2 (g) ? 2 HBr (g),

K = 4.0 x 10-2.

For the reaction :: 2 HBr (g) ? H2 (g) + Br2 (g)

K =:

a. 4.0 x 10-2

b. 5

c. 25

d. 2.0 x 10-1


24. Does the pH of a solution increase, decrease, or stay the same when you add solid ammonium chloride to a solution of 0.10 M NH3?


35. Classify each reactant as either a Bronsted-Lowry acid or base for the following reactions:

a)      HCN + H2O  ? CN- + H3O+

b)      CH3NH2 + H2O  ? CH3NH3+ + OH-

46. How many times more acidic is a solution with pH = 4.80 as compared to one with pH = 6.33?


(please explain/show work)


Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2...
Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2 x 10-10). Which of the following statements is true? a) The solution is not a buffer because [HCN] is not equal to [CN-] b) The pH will be below 7.00 because the concentration of the acid is greater than that of the base. c) [OH-] > [H+] d) The buffer will be more resistant to pH changes from addition of strong acid than to...
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr...
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr and 0.130 M in HCHO2 b) A 0.25 M CH3NH3I solution? (Kb = 4.4 x 10-4 M for CH3NH2) c) A 0.0180 M solution of HClO2? (Ka = 1.1 x 10-2 M) d) A 0.0180 M solution of Sr(OH)2 e) A 0.170 M solution of KOCl? (For HOCl, Ka = 3.5 x 10-8 M) f) A solution that is 3.00×10−2M in HI and 9.00×10−3M...
1. A certain solution has a concentration of 1.0 x 10-4 M of OH-. Which of...
1. A certain solution has a concentration of 1.0 x 10-4 M of OH-. Which of the following statements is true? Select one: A. The solution has a pH of 10. B. The solution is acidic. C. The solution has a pH of 4. D. The solution has a H+ concentration of 1.0 x 10-4 M as well. 2. How do you know an acid is weak? Select one: a. It does not totally dissociate in water, setting up a...
18. Which H3O+ concentration and classification (acidic vs. basic) are correctly matched for a solution in...
18. Which H3O+ concentration and classification (acidic vs. basic) are correctly matched for a solution in which the OH- concentration is 5.6 x 10-6 M? a. 5.6 x 10-6 M : basic b. 5.6 x 10-6 M : acidic c. 5.6 x 108 M : acidic d. 1.8 x 10-9 M : basic e. 1.8 x 10-9 M : acidic 19. The solution that will give a pH = 12.00 is (MW: NaOH = 40 g/mol): a. 4.0 g NaOH...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl and 0.2 M NH3 (Ka for NH4Cl = 5.6 x 10-10). Assume 2 significant figures in all of the given concentrations so that you should calculate all of the following pH values to two decimal places. 1. Calculate the pH of this solution. 2. Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on...
what is the [H3O+] of a solution with a pH 1.26? Input answer in scientific notation...
what is the [H3O+] of a solution with a pH 1.26? Input answer in scientific notation with E representing x 10. For example, the number 8.4 x 10-4 would be entered as 8.4E-4. Calculate the value of the equilibrium constant, K, using the reaction below and the given concentrations at equilibrium. Answer using two significant figures. H2 (g) + Cl2 (g) ↔ 2 HCl (g) [ H2] = 0.75 M [ Cl2] = 0.96 M [ HCl] = 6.0 M...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...
When a 27.2 mL sample of a 0.371 M aqueous hydrocyanic acid solution is titrated with...
When a 27.2 mL sample of a 0.371 M aqueous hydrocyanic acid solution is titrated with a 0.316 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH = note Acid/Base Ionization Constants at 25 oC Acid Formula Ka1 Ka2 Ka3 Acid/Base Ionization Constants at 25 oC Acid Formula Ka1 Ka2 Ka3 Acetic acid CH3COOH 1.8×10-5 Acetylsalicylic acid (aspirin) HC9H7O4 3.0×10-4 Aluminum ion Al(H2O)43+ 1.2×10-5 Arsenic acid H3AsO4 2.5×10-4 5.6×10-8 3.0×10-13 Ascorbic acid H2C6H6O6...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
Can you please check my answers and tell me if they are correct? thanks 8. Write...
Can you please check my answers and tell me if they are correct? thanks 8. Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds: (a) PbCl2       PbCl2(s) --> Pb2+(aq) + 2Cl-(aq)                           Ksp = [Pb2+][Cl-]2   (b) Ag2S        Ag2S(s) --> 2Ag+(aq) + S2-(aq)                             Ksp =[Ag+]2[S2-] (c) Sr3(PO4)2 Sr3(PO4)2(s) --> 3Sr2+(aq) + 2PO43-(aq)         Ksp =[Sr2+]3[PO43-]2 (d) SrSO4       SrSO4(s) --> Sr2+(aq) + SO42-(aq)                       Ksp =[Sr2+][SO42-] 14. Assuming that no equilibria other than dissolution are involved,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT