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
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Chemistry: Atoms First
- 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_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
- A 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_forwardDetermine 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_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
- (a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.arrow_forwardWrite the expression for K, and K, for the reaction PH;BCl,(s) = PH;(e) + BCl(g) 1.arrow_forward6. (a) Write an equation where calcium acetate is adding to water. (b) Looking at the equation in (a), is this salt acidic, basic or neutral? (c) Determine the pH of a solution of calcium acetate, Ca(CH₂COO), that is 0.275 M. (Ka for CH₂COOH is 1.8 x 105).arrow_forward
- The propionate lon, CHCH,COO", reacts with water as a weak base: CHCH,COO", (aq) + H2O() = CH,CH,COOH(aq) + OH"(ag), with K-7.4x 10 1o at 25°C. If sodium propionate were dissolved in water to make a 0.80M solution, what would be the resulting concentration of OH"? Type your answer.arrow_forwardThe acid dissociation constants for sulfurous acid are: Ka1 3D 1.2 х 10-2 and Ka2 - 6.6 х 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.arrow_forwardCalculate the pH of each of the following solutions (b) a solution that is 0.115 M in NaCIO and 0.0450 M in KI; (c) a solution that is 0.00165 M in HCl and 0.0150 M in HCIO2; (d) a solution prepared by mixing 15.0 mL of 17.5 M acetic acid with 8.54 g of sodium acetate and diluting to a total volume of 1.25 L;arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning