Concept explainers
(a)
Interpretation: The expected osmotic pressure of the given solution of
Concept introduction: Osmotic pressure is the amount of pressure required to be applied across a semi-permeable membrane in order to stop the flow of solvent molecules in a solution of lower concentration to higher concentration. Osmotic pressure is a colligative property. The value of osmotic pressure is calculated by the formula.
To determine: The expected osmotic pressure of the given solution of
(b)
Interpretation: The expected osmotic pressure of the given solution of
Concept introduction: Osmotic pressure is the amount of pressure required to be applied across a semi-permeable membrane in order to stop the flow of solvent molecules in a solution of lower concentration to higher concentration. Osmotic pressure is a colligative property. The value of osmotic pressure is calculated by the formula.
To determine: The value of
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Chemistry: An Atoms First Approach
- Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.arrow_forwardProve that Ka3 Kb1 = Kw for phosphoric acid, H3PO4, by adding the chemical equilibrium expressions that corresponds to the third ionization step of the acid in water with the first of the three successive steps of the reaction of phosphate ion, PO43, with water.arrow_forwardIonization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 102. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.arrow_forward
- 1) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures?arrow_forward. The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. Write the chemical equation for the ionization of this acid in water. Write the Ka expression for this acid. What is the equilibrium concentration of each product and the reactant?arrow_forwardBoric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solutionof boric acid? What is the degree of ionisation of boric acid in this solution? Thehydrogen ion arises principally from the reaction:B(OH)3(aq) + H2O(l) B(OH)4(aq)_+ H+(aq)The equilibrium constant for this reaction is 5.9x10-10arrow_forward
- A weak acid, HA, is a monoprotic acid. A solution that is 0.220 Min HA has a pH of 2.440 at 25°C. HA(aq) + H2O(1) H30¯(aq) + A¯(aq) What is the acid-ionization constant, K. for this acid? What is the degree of ionization of the acid in this solution? Ka= Degree of ionization: =arrow_forwardWhat is the equilibrium constant for the ionization of the HSO4− ion, the weak acid used in some household cleansers: HSO4−(aq) + H2 O(l) ⇌ H3 O+(aq) + SO42−(aq)In one mixture of NaHSO4 and Na2SO4 at equilibrium, [H3 O+] = 0.027 M; [HSO4−] = 0.29 M; and[SO42−] = 0.13 M.arrow_forward15) 0.28 grams of sodium hydroxide are added to 40.0 mL of 0.25 M formic acid. Calculate the pH of the resulting solution. K, for the formate ion = 5.88 x 10-1.: * A) 3.40 B) 4.14 C) 9.83 D) 10.57arrow_forward
- Boric acid, BOH is used as a mild antiseptic. What is the PH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction: B(OH)3(aq) + H2O(l) > B(OH)4- (aq) + H+ (aq) The equilibrium constant for the reaction is 5.9 x10-10arrow_forwardAmmonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- Calculate the equilibrium constant for this reaction (the reaction goes from left to right) at 25 ºC. ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/molarrow_forwardA 0.60M solution of NH 3 is prepared and is in equilibrium with its ions. Calculate the followingwith K b = 1.8x10 -5(a) Concentrations of hydrogen ions in the solution?(b) Degree of Ionizationarrow_forward
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