Concept explainers
Interpretation:
Among the given graphs, the graph that best represents the relationship between pH of a acidic salt solution and the
Concept Information:
Base ionization constant
The equilibrium expression for the ionization of weak base
Where
pH and pOH:
The pOH scale is the reverse of pH scale
To Explain: The diagram that best represents the relationship between pH of a acidic salt solution and
Want to see the full answer?
Check out a sample textbook solutionChapter 16 Solutions
CHEMISTRY:ATOMS FIRST (LL)>CUSTOM PKG.<
- A biology experiment requires the use of a nutrient fluid buffered at a pH of 4.85, and 659 mL of the solution is needed. It has to be buffered to be able to hold the pH to within =0.10 pH units of 4.85 even if 5.00 x 10 mol of OH or 5.00 x 10 mol of H* ion enter. Record all your answers to three (3) significant figures. Pick the best acid and its sodium salt that could be used to prepare the solution. O Hydrocyanic acid and sodium cyanide (pK, = 9.21). O Nitrous acid and sodium nitrite (pk, = 3.15). Acetic acid and sodium acetate (pK, = 4.74). O Hydrofluoric acid and sodium fluoride (pK, = 3.17). Hint Calculate the minimum number of grams of the acid and its sodium salt that are needed to prepare the buffer solution. Mass acid i Mass sodium salt = i Hint Calculate the molar concentration of the acid and its sodium salt that are needed to prepare the buffer solution. Concentration acid = M Concentration sodium salt = M Hint onarrow_forward13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is the pH of the solutionafter 10.00 ml of HCl is added?(a) 4.19(b) 5.09(c) 5.74(d) 6.2414. What is the ratio of moles of benzoate (C7H5O2‒) to benzoic acid (HC7H5O2) in the solution that results from thecombination of the NaC7H5O2 and HCl in the problem above?(a) 8(b) 0.125(c) 0.0040(d) 0.00050arrow_forward(a) Calculate the acetate ion concentration in a solution prepared by dissolving 8.70×10-3 mol of HCl(g) in 1.00 L of 1.10 M aqueous acetic acid (Ka = 1.80×10-5). (b) Calculate the pH of the above solution. Give your answer to two decimal places.arrow_forward
- B ONLY (a)How many ml of 0.5 M HCl must be added to 100.0 ml of a 0.2 M Imidazole (C3H4N2 ; Kb=6.3x10-8) solution to obtain a pH of 5.52? (b)Is this solution a buffer?arrow_forwardPropionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.arrow_forwardThe major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forward
- The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are told the liquid ispure water, a solution of HCl(aq), or a solution of KOH(aq).Which one is it? (b) If the liquid is one of the solutions,what is its molarity? (c) Why is the temperature given onthe pH meter?arrow_forwardThe ion HTe− is an amphiprotic species; it can act as either an acid or a base.(a) What is Ka for the acid reaction of HTe− with H2O?(b) What is Kb for the reaction in which HTe− functions as a base in water?(c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe−] in a 0.10 M solution of H2Te.arrow_forwardA student is provided with a 0.1 M stock solution of NaOH. Student was then asked to mix 50.0 mL of this stock solution of NaOH with 450.0 mL of water to prepare a dilute solution of NaOH. (A) Calculate the molarity of the diluted solution. (B). Calculate the hydronium ion concentration, [H3O+] in the final diluted solution. (8 points) (C ) Calculate the pH of the diluted NaOH solution. (D) Is the final diluted solution acidic, basic or neutral?arrow_forward
- 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).arrow_forwardA solution is prepared at 25 °C that is initially 0.057M in dimethylamine ((CH3), NH), : a weak base with K,=5.4 × 10 and 0.29M in dimethylammonium bromide ((CH,), NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. 2 pH = |||arrow_forwardIf the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity constant, Kp, of CICH20-? You do not need to make a simplifying assumption CICH,0-(aq) + H2O(1) СICH-OОH(aq) + ОН (аq) K½ = ?arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning