Acid/Base Equilibria - Example 5 Calculate the concentrations of H₂SO4, HSO4 and H+ ions in 0.14 mol L-1 aqueous sulfuric acid solution at 25°C. The acidity constants are Ka,1 = ∞ and K₂,2 = 0.013. Solution

Acid/Base Equilibria - Example 5 Calculate the concentrations of H₂SO4, HSO4 and H+ ions in 0.14 mol L-1 aqueous sulfuric acid solution at 25°C. The acidity constants are Ka,1 = ∞ and K₂,2 = 0.013. Solution

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 107QAP: What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2,...

See similar textbooks

Related questions

Q: 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: (a) Initial Concentration of CH3COOH Given mass of acetic acid = 0.056 gms, Volume of…

Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H,O(1) =…

A: The equilibrium constant Ka expresses the relation between products and reactants of a reaction at…

Q: 11.An acid-base equilibrium system is created by dissolving 0.15 mol HNO2 in water and diluting the…

A: pH change before addition:

Q: The pH of an aqueous solution of 0.291 M ammonium perchlorate, NH4ClO4 (aq), is This solution is -5…

A: Concentration of NH4ClO4 = 0.291 MKb of NH3 = 1.80×10-5

Q: A monoprotic weak acid,HA, dissociates in water according to the reaction HA(aq)+H2O equilibrium…

Q: Calculate the hydronium ion concentration and pH of a 0.045 M solution of chloroacetic acid. (Ka =…

Q: Calculate the pH of 1.0 M hydrazinium chloride, N2H5CI. For hydrazine, N2H4, Kp = 1.3 x 106. pH =…

Q: 8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a…

Q: The ionization constant of lactic acid, CH;CH(OH)CO,H, an acid found in the blood after strenuous…

Q: Calculate the pH at 25 °C of a 0.30M solution of potassium acetate (KCH,CO,). Note that acetic acid…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of…

A: The acid-base equilibrium between CH3COOH and H2O is given by the reaction.

Q: Calculate the equilibrium constant for the following reaction: CH3COOH(aq) + F (aq) =CH₂COO (aq) +…

A: The known values are as follows:Ka of CH3COOH = 1.8× 10-5Ka of HF = 6.8×10-4

Q: Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates,…

A: The equilibrium constant (Kc) of the equation in which divide the product concentration terms with…

Q: Calculate the pH of a solution prepared by dissolving 0.482 mol of benzoic acid and 0.104 mol of…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Lakes have a natural buffering capacity, especially in regions where limestone gives rise to…

A: Sulphuric acid in the lake contains H3O+ ions. when acid rain falls in the lake that contains…

Q: A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M…

A: The pH of NaA solution = 9 The concentration of NaA = 0.050 M pOH = 14-9 = 5 pOH = - log…

Q: One strategy for dealing with the acidification of lakes is periodically to add powered limestone…

A: Solution - According to the question - Given - Ksp expression for CaCO3 is Ksp = [Ca2+] [CO32-]…

Q: For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) = H,NNH3* (aq) + OH (ag) K, is…

Q: For the titration of an aqueous nitrous acid solution, HNO (ag), with an aqueous strontium hydroxide…

A: The expected pH for the titration of HNO2 and Sr(OH)2 is to be determined. The equivalence point…

Q: Calculate the pH at 25 °C of a 0.87M solution of potassium butanoate (KC,H,CO,). Note that butanoic…

A: For salt of weak acid strong base C3H7CO2H + KOH →C3H7CO2K + H2O weak acid strong base pH =…

Q: Calculate the pH at 25 °C of a 0.92M solution of potassium butanoate (KC,H,CO,). Note that butanoic…

A: Dear student I have given answer to your question in the image format.

Q: Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH? O…

A: The objective of the question is to determine the solution with the lowest pH.

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: Sodium lactate is the sodium salt of lactic acid. a) Use Acid-Base Properties of Salt Solutions, to…

Q: Human blood has a pH of approximately 7.4 due to the carbonic acid/bicarbonate ion (H2CO3/HCO3−)…

A: #(i): The given reaction for the dissociation of H2CO3 is H2CO3(aq) ⇌ CO2(g) + H2O(l)

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (CH3O;)? CsH2Or(aq) +…

Q: 3.134 grams of potassium sorbate (KCH3(CH,)4CO2 ) is fully dissolved in 100.00 mL of water, which is…

Q: 5) Find the concentration of H3O*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka=…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: Write the equilibrium constant expression, K, for the following reaction taking place in dilute…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: The salt given is KC3H5O3.

Q: Calculate the pH and the equilibrium concentrations of HS and S2 in a 0.0805 M hydrosulfuric acid…

Q: Calculate the pH at 25 °C of a 0.44M solution of potassium butanoate (KC,H,CO,). Note that butanoic…

A: Given- Concentration of potassium butanoate= 0.44M pKa of weak acid=4.82 Temperature =…

Q: When the reversible reaction HC;H;0, (aq) > H'(aq) + C;H;O2(aq) is at equilibrium at room…

A: (1). pH of reaction mixture = 5 Reaction is reversible in nature, Large amount of sodium hydroxide…

Q: Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in…

A: GivenpH of propanoic acid solution=2.96 H+ ion concentration in the solution can be calculated by…

Question

No
s
32
Acid/Base Equilibria - Example 5
Calculate the concentrations of H₂SO4, HSO4 and H+ ions in 0.14 mol L-1
aqueous sulfuric acid solution at 25°C.
The acidity constants are Ka,1
and Ka2 = 0.013.
Solution
32
=∞

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

CONCLUSION

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Consider the weak bases below and their Kp values: NH3 Ky = 1.8 x 10-5 C2H5NH2 Kp = 5.6 x 10-4 C5H5N Kp = 1.7 x 10-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength. O CsH;NH< NH,*< C2H5NH3* C2H5NH;*= NH,= C5H5NH* C2H5NH3*< NH4*< C5H5NH* O NH,*< C,H5NH;*
What is the pH at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s law constant forCO2 at 25 °C is 3.1 x 10-2 mol/L-atm.
P Please don't provide the handwriting solution
Calculate the equilibrium Molarity of HPO4^2-
Suppose a 0.17 Maqueous solution of phosphoric acid (H,PO) is prepared. Calculate the equilibrium molarity of HPO, You'l find information on the 2- properties of phosphoric acid in the ALEKS Data resource. Round your answer to 2 significant digits.
Calculate the concentrations of all species present (other then water) in an aqueous solution of 0.25 M H2SO3 Constants: Ka1,H2SO3= 1.5x10^-2 Ka2,H2SO3= 6.3x10^-8 Kw= 1.0x10^-14
The lactate ion, C, H,O, (aq), reacts with water to form lactic acid and hydroxide ion. C;H,05 (aq) + H, O(1) = HC,H;O;(aq) + OH (aq) In a 0.378 M solution of sodium lactate, the [OH¯] = 5.2 × 10-6 M. Use the ICE table to determine the concentrations of OH¯ and HC, H,O,. You will use these values to calculate the Kp for HC,H,O3. C;H;O5 (aq) + H,O(1) = HC,H;O,(aq) + ОН (аq) initial 0.378 change +x +x equilibrium 0.378 – x What is the value for x in these expressions? Hint: you are given this value in the problem. x = M
Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go down
In water, the equilibrium 2H2O(l) ⇄ H3O+(aq) + OH−(aq) Kc = 10-14 determines the concentrations of H3O+(aq) and OH−(aq). If the pH is 9.2, what is the OH− concentration? (H3O+(aq) and H+(aq) are equivalent ways of representing a solvated proton).
2- Suppose a 0.024M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium molarity of HPO properties of phosphoric acid in the ALEKS Data resource. You'll find information on the Round your answer to 2 significant digits. OM x10
A diprotic acid, H, A, has acid dissociation constants of K,j = 1.45 x 10-4 and K2 = 5.12 x 10-". Calculate the pH and molar concentrations of H,A, HA, and A²- at equilibrium for each of the solutions. A 0.184 M solution of H,A. pH = 2.2865 [H,A] = 0.1788 [HA"] = 5.17 xI10-3 [A?-] = M 5.12 x10-11 M A 0.184 M solution of NaHA. pH= [H,A] = M. [HA-] = [A2-] = M M