Determine the pH of each of the following solutions. (a) 0.762 M hypobromous acid (weak acid with Ka = 2.5e-09). (b) 0.558 M hydrosulfuric acid (weak acid with Ka = 9.5e-08). (c) 0.543 M pyridine (weak base with Kb = 1.7e-09).

Determine the pH of each of the following solutions. (a) 0.762 M hypobromous acid (weak acid with Ka = 2.5e-09). (b) 0.558 M hydrosulfuric acid (weak acid with Ka = 9.5e-08). (c) 0.543 M pyridine (weak base with Kb = 1.7e-09).

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

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 7P

See similar textbooks

Related questions

Q: A large volume of 0.1760 M H2SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution…

A: Introduction: pH: pH is used to express the acidity of the solution. It is defined as negative…

Q: If the pKa of HCIO is 7.46 and the pH of an HCIO/NaCIO solution is 7.59, O [HCIO]>[CIO] O…

Q: d. During the fermentation of wine, a buffer system consisting of tartaric acid and potassium…

A: Given that, during the fermentation of wine, a buffer system consisting of tartaric acid and…

Q: Write the whole acid base equation for the reaction of KOH(aq) with HC4H7O2(aq) b) write the net…

A: (a) Acid base equation KOH(aq) + HC4H7O2(aq) → KC4H7O2(aq) + H2O (l) (b) Net ionic…

Q: Using paleolimnological methods it is possible to estimate past pH values of surface waters. If the…

A: Solution: Given that pH of surface water using paleolimnological method is 5.787 So, pH = -log[H+]…

Q: The pH of a solution containing a [H3O+] = 3.40 x 10 negative 5 M, is:

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: The pH of an aqueous solution of 0.134 M sodium fluoride, NaF (aq), is This solution is

A: Answer:- This question is answered by using the simple concept of calculation of pH of aqueous…

Q: What is the pH of a 0.0810 M solution of HONH;CI (Kb of HONH2 is 1.1 x 108)?

A: Given, HONH3Cl -----> HONH3+ + Cl- Hydrolysis of the weak conjugate acid, HONH3+…

Q: Determine both the pH and the % ionization of a 0.53 M hypochlorous acid, HCIO, solution at 25°C.…

A: The given data is as follows: The concentration of HClO = 0.53 M The value of Ka for HClO = 2.9×10-8…

Q: Calculate the pH of a solution that is prepared by dissolving 0.23 mol of hydrofluoric acid (HF) and…

Q: Suppose a 0.48M aqueous solution of phosphoric acid (H,PO,) is prepared. Calculate the equilibrium…

A: Given, Concentration of aqueous Phosphoric acid solution = 0.48 M Required,…

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: 7. The pH of a 0.10 M solution of acetic acid (CH3COOH) is 2.39. What is the Ka of acetic acid?

A: H3O+ can be calculated as follows: pH=-log [H3O]+[H3O]+=10-pH[H3O]+=10-2.39[H3O]+=0.00407 M

Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a)…

A: Given The acid-dissociation constant (Ka) for hypochlorous acid is 3.0 x10-8. The initial…

Q: What is the pH of a 0.540 M solution of Ca(NO,), (Ka of HNO, is 4.5 x 10*)?

Q: Suppose a 0.031 Maqueous solution of phosphoric acid (H, PO) is prepared. Calculate the equilibrium…

Q: The pH of an aqueous solution of 9.43x102 M tellurous acid, H,TeO3 (aq), is For H,TeO3 K =5.40*10…

A: Dissociation of tellurous acid is, Ka1 and Ka2 values of a tellurous acid are given as 5.40×10-7…

Q: the pH of an acid solution is 3.59. If the concentration of the acid in the solution is 0.200 mol/L,…

A: Given Concentration of the acid=0.2 mol/LpH of the acid solution=3.59Ka of thel acid=??

Q: Determine the pH of a 0.461 M C3H5CO,H M solution if the K, of C6H5CO2H is 6.5 x 105. 4.52 11.74…

A: pH is commonly known power of hydrogen, it measures the concentration of hydrogen ion in the…

Q: A weak base is dissolved in water with a concentration of 0.200 mol/L. The Kb value of the base is…

A: Given :- initial concentration of base = 0.200 mol/L Kb of base = 9.75 × 10-4 To…

Q: The pH is measured to be 2.58 for a solution of 0.035 M cyanic acid, HOCN (aq). Write the hydrolysis…

A: HOCN is a weak acid. Weak acid are those acid which does not dissociates completely in equilibrium.…

Q: What is the pH of a 0.870 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Answer:- This question is answered by using the simple concept of hydrolysis of the salt formed by…

Q: The Ka value for acetic acid, CH3COOH(aq), is 1.8×10−5. Calculate the pH of a 2.80 M acetic acid…

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: Suppose a 0.48M aqueous solution of phosphoric acid (H,PO,) is prepared. Calculate the equilibrium…

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: A study of the acid shows that the pH of an acid HA O.12 MIK2.62. What is the K, of this acid?

A: Acid Dissocaition constant, Ka has to be determined for the Acid HA of 0.12 M with pH 2.26.

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

A: The dissociation of formic acid. Given data: Initial concentration of formic acid is 0.558M. pH of…

Q: Q3// The basicity constant Kp for ammonia is 1.75 x 10 at 25°C. Calculate the pH and pOH for a 1.00…

A: As per our guidelines we can only solve first question. Please resubmit the other questions as next…

Q: The molar concentration of H3O+ ions in the following solutions was measured at 25 °C. Calculate the…

A: pH is used to measure acidity or basicity of an aqueous solution. pH of any solution can be…

Q: What is the pH of a 0.380 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: When acidulated water (dil.H2SO2solution) is electrolysed, will the pH of the solution be affected?…

A: Anode reaction is given

Q: The pH of an aqueous solution of 0.0103 M hydrosulfuric acid, H2S (aq), is

A: Given, Molarity of H2S = 0.0103 M First acid dissociation constant of H2S = Ka1 = 1.0 x 10-7…

Q: Hypobromous Acid, HOBr, and hypoiodous acid, HOI are both weak acids. Which acid is stronger and…

A: Hypohalous acids tend to be weak acids and they tend to get weaker as the halogen progresses further…

Q: Chemists working with fluorine and its compounds some- times find it helpful to think in terms of…

A: (a) would the acid in this system be the fluoride donor or fluoride exceptor (b) Identify the acid…

Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D) 0.100…

Q: A 0.539 M solution of oxalic acid (pK, = 1.23) is prepared. Determine the pH of the !3! solution.…

Q: Below is the reaction for the formation of acid rain due to high concentration of atmospheric…

A: Given reaction is : CO2 (g) + H2O (l) <---------> H2CO3 (aq) pH = 3.5 What is the…

Q: The [H3O+] of Coca-Cola Classic ® is 3.2 x 10-3. What is its pH? Is it acidic or basic?

A: The pH of the given solution can be defined as the measure of its basicity or the acidity. It is…

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO, =…

Q: A major component of coral is carbonate ions, which is created by the dissociation of bicarbonate…

A: Here we are required state effect on the concentration of carbonate when acidity is increased

Q: Would you expect an aqueous solution of manganese (VII) oxide to have a ph greater or less than 7.0?…

A: Oxidation state is the number of electrons that are either gain or lose by an atom in a chemical…

Q: Determine the pH of each of the following solutions. (a) 0.829 M hydrazoic acid (weak acid with Ka =…

Question

Determine the pH of each of the following solutions.

(a) 0.762 M hypobromous acid (weak acid with K_a = 2.5e-09).

(b) 0.558 M hydrosulfuric acid (weak acid with K_a = 9.5e-08).

(c) 0.543 M pyridine (weak base with K_b = 1.7e-09).

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Determine the pH of each of the following solutions.(a) 0.684 M hypochlorous acid (weak acid with Ka = 3e-08).(b) 0.399 M hydrogen peroxide (weak acid with Ka = 2.4e-12).(c) 0.751 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.134 M hypochlorous acid (weak acid with Ka = 3e-08). (b) 0.283 M hydrazoic acid (weak acid with Ka = 1.9e-05). (c) 0.879 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions.(a) 0.112 M acetic acid (weak acid with Ka = 1.8e-05).(b) 0.855 M hydrazoic acid (weak acid with Ka = 1.9e-05).(c) 0.867 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions.(a) 0.246 M hydrocyanic acid (HCN) (weak acid with Ka = 4.9e-10).(b) 0.228 M propionic acid (weak acid with Ka = 1.3e-05).(c) 0.850 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.826 M hydrocyanic acid (HCN) (weak acid with K₂ = 4.9e-10). 5.81 (b) 0.656 M hypobromous acid (weak acid with K₂ = 2.5e-09). (c) 0.673 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions.(a) 0.257 M hypobromous acid (weak acid with Ka = 2.5e-09).(b) 0.809 M ascorbic acid (weak acid with Ka = 8e-05).(c) 0.555 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following solutions. (a) 0.296 M arsenous acid (weak acid with Ka = 5.1e-10). (b) 0.315 M boric acid (weak acid with Ka = 5.8e-10). (c) 0.571 M pyridine (weak base with Kb = 1.7e-09).
The pH scale for acidity is defined by pH – log10 H*| where |H*| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of rain water is 5.5. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M
Determine the pH of each of the following solutions. (a) 0.549 M hydrogen peroxide (weak acid with Ка 3 2.4e-12). (b) 0.615 M acetic acid (weak acid with Ka 1.8e-05). (c) 0.866 M pyridine (weak base with Kp = 1.7e- 09).
4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂
6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =