Calculate the pH, pOH, and the fraction of protonated acid for the 0.1 M solution of lactic acid (see Table 4.4 for pK, values, also attached below).
Q: An unknown weak base (B) undergoes reversible dissociation in water according to the following…
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Q: For a solution of 0.020 M lactic acid, HC3H5O2 (Ka = 8.4 × 10-4), calculate: [H+]= _______ M pH=…
A: For a weak acid ,HClO HC3 H5O2 ⇌ C3 H5O2 - + H+…
Q: Calculate the pOH of the following aqueous solutions at 25°C: (a) 0.013 M LiOH, (b) 0.013 M Ba(OH)2…
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Q: A. What is the pOH of the solution at the half equivalence point? B. What is the ionization…
A: Given data : Unknown base solution = 10 ml . Titrated with known concentrated HCl of molar…
Q: A solution is prepared at 25 °C that is initially 0.15M in acetic acid (HCH,CO,), a weak acid with…
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Q: What is the pHpH of a 0.24 M0.24 M solution of the weak base?
A: pH + pOH = 14 pH = 14 - pOH pOH = -log[OH-]
Q: Using the systematic approach, calculate for the pH of the following aqueous solutions at 25°C: a.…
A: Since you have posted a question with multiple sub-parts, we will solve first three subpartsfor you.…
Q: HA is a weak acid which is 4.0% dissociated at 0.100M. Determine the Ka for this acid.
A: HA is a weak acid so it dissociate partially
Q: Calculate the pH of a solution prepared by mixing 0.0660 mol of chloroacetic acid plus 0.0110 mol of…
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Q: 0.1 M Na2CO3 solution, using the given pH data, write net-ionic equation for hydrolysis:
A: Net ionic equation for hydrolysis reaction has a general form given below: An ion +…
Q: Reverse the concentrations of the weak acid and conjugate base for 0.25 M HC2H3O2 and 0.030 M…
A: Case 1: Concentration of weak acid and conjugate base are as follows: [CH3COOH] = 0.25 M [CH3COONa]…
Q: 0.1 M Na2CO3 solution, using the given pH data, write expression for equilibrium constant (Ka or…
A: As the pH of Na2CO3 is 11.0 which means that it is basic in nature.
Q: (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.074 M aqueous…
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Q: A 0.137 M solution of a weak base has a pH of 11.36. What is the base hydrolysis constant, ?b, for…
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Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively…
A: Kh=kWkC pH + pOH = 14 From Ostwald's dilution law , pOH=-logkbxc Where c is the concentration of…
Q: For each solution, determine the [H3O*], [OH], and pH. Show problem set ups and set the answers with…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is 2320.1 kJ/mol. (a)…
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Q: The pH of an aqueous acid solution is 6.15 at 25°C. Calculate the K, for the acid. The initial acid…
A: Given :- initial concentration of acid = 0.012/M pH of solution = 6.15 To calculate :- Ka of…
Q: Grams of Sodium Formate required to add to 400ml of 0.1M Formic acid to make the pH of solution by…
A: The reaction can be given as follows: HCOOH(aq)+NaOH(aq)→HCOO-Na+(aq)+H2O(l) Molarity of formic acid…
Q: Calculate the pH, the pOH, and the molarity of all species in solution for a 2.45 M butanoic acid…
A: Given :- molar concentration of butanoic acid = 2.45 M To calculate :- Molarity of all species…
Q: Calculate the pH of a 0.15M solution of sodium acetate (CH3COONa). What is the percent hydrolysis?…
A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…
Q: A solution is prepared at 25 °C that is initially 0.27 M in acetic acid (HCH,CO,), a weak acid with…
A: Given that : Concentration of acetic acid (acid) = 0.27 M Concentration of sodium acetate (salt) =…
Q: A solution is prepared at 25 °C that is initially 0.43 M in propanoic acid (HC,H,CO,), a weak acid…
A: Given :- [HC2H5CO2] = 0.43 M [KC2H5CO2] = 0.11 M Ka for HC2H5CO2 = 1.3 × 10-5 To calculate :-…
Q: Calculate the degree of ionization of a 0.05F solution of lactic acid.
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Q: 0.1 M NaC2H3O2 solution, using the given pH data, write net-ionic equation for hydrolysis:
A: Hydrolysis net ionic equation has the general form as: An ion + water-----> a molecule or ion +…
Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10¯'. Calculate the pH of a 3.3…
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Q: A solution is prepared at 25 °C that is initially 0.37 M in nitrous acid (HNO,), a weak acid with K,…
A: Since the pH of monoprotic acid buffer is given by Henderson-Hasselbalch equation as where pKa =…
Q: A 0.825 M solution of a weak base has a pH of 11.83. What is the base hydrolysis constant, ?b, for…
A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…
Q: 2. The pH of a 0.100 M weak acid solution is 4.07. Calculate the K, value for the weak acid.
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: Show complete calculations for the pH of a 0.125M solution of acetic acid. The K, for acetic acid is…
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Q: A solution is prepared at 25 °C that is initially 0.051M in benzoic acid (HC,H,CO,), a weak acid…
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Q: Based on the pH, determine [OH ] at equilibrium for this weak base solution. Express your answer to…
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Q: A solution is prepared at 25 °C that is initially 0.12M in acetic acid (HCH,CO,), a weak acid with…
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Q: Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine…
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Q: A weak base has a base hydrolysis constant, ?b, of 2.8×10−6. What is the pH of a 0.15 M solution of…
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Q: Calculate the pH of a 1.00L solution which is made up of 0.058 mol acetic acid and 0.030 mol sodium…
A: Given: Moles of acetic acid i.e. CH3COOH = 0.058 mol. Moles of sodium acetate i.e. CH3COONa = 0.030…
Q: Calculate for the [H+] of an oxalic acid solution with a pH of 4.7. What is the pOH and [OH-] of the…
A: We have given that pH = 4.7 We know that pH = -log[H+] [H+] = 10-4.7 = 2.0×10-5
Q: A 0.861 M solution of a weak base has a pH of 11.80. What is the base hydrolysis constant, K, for…
A: Hydrolysis constant Kb can be calculated by the following way .
Q: Calculate the pOH of a solution that contains 7.8 x 10-6 M OH⁻ at 25°C.
A: pOH can be calculated using the given formula.
Q: What is the range of pH? Ph could be less than zero for strong acid solution and more than 14 in…
A: pH is the measure of how acidic or basic a solution is. A solution with high number of hydroxide…
Q: Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH,)…
A: The weak base given is (CH3)2NH Since weak base reacts with water to produce conjugate acid and…
Q: Determine the pH of a 0.100 M solution of butanoic acid, whose percent deprotonation (aka percent…
A: The dissociation of butanoic acid is as follows: CH3CH2CH2COOH <--------->CH3CH2CH2COO-(aq) +…
Q: 4. You are given 1.500 M of HC1O,, Ką = 1.1 × 10² at 25°C. Determine its pH.
A: SOLUTION: Step 1: Since HClO2 has a low Ka value, it is a weak acid. Weak acids partially dissociate…
Q: Calculate the ph and poh for a solution that is 0.63 M in NH3 and 0.4 M in NH4Cl, Ki for NH3 is…
A: Given, The molarity of NH3 = 0.63 M The molarity of NH4Cl = 0.4 M The Ki for NH3 = 1.9 × 10-5 The…
Q: The OH– concentration in a solution of 0.0100 M NaClO is 5.9×10–5 M. What is the value of Kb for…
A: The OH- concentration in a 0.01 M solution of NaClO has been provided.
Q: A solution is prepared at 25 °C that is initially 0.28M in propanoic acid (HC,H,Co,), a weak acid…
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Q: Determine the pH of an HF solution of each of the following concentrations. (Ka for HF is 6.8×10−4)…
A: HF is a weak acid, hence it only dissociates partially. ICE table is given by, HF H3O+…
Q: Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine…
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- (a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .Calculate the pH for a mixture of one mole of benzoic acid andone mole of sodium benzoate. The pKa of benzoic acid is 4.2.Phosphoric acid is a tri-acid. It is often associated to biological molecules (i.e. proteins, lipids) in the form of phosphate group. Its ionisation state depends on the pH of the solution and of its pKa values. Data: pka₁ = 2.1; pKa₂ = 7.2 ; pka3 = 12.4 1- What are the forms present at physiological pH (7.4) ? 2- Indicate which form is the most prominent.
- What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…L-lactate is constantly produced from pyruvate via the enzyme lactate dehydrogenase (LDH) in a process of fermentation during normal metabolism and exercise. It can pick up a proton and become lactic acid(see right). The pK, of lactic acid is 3.86. A) Identify the ionizable oxygen that is partially protonated (50 % dissociated) at pH=3.86. ÕH B) Determine the acid dissociation constant, (Ka)?Like any equilibrium constant, Kw changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T ? Explain with a reaction that includes heat as reactant or product. (b) In many medical applications, the value of Kw at 37°C (body temperature) may be more appropriate than the value at 25°C, 1.0 x 10-14. The pH of pure water at 37°C is 6.80. Calculate Kw, pOH, and [OH-] at this temperature.
- (a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.نقطتان )2( The pH of a 1.00 M Solution -1 of Nitrous acid HNO2 (pKb =10.6) isThe Ka of a weak acid is 3.33 x 10-5, what is the pKb of it's conjugate base?
- . (a) Combine the following equations to construct an acid-base reaction equation, in the process drawing complete Lewis structures for both reactants and products, along with arrows to show the movement of nonbonded electrons. (b) Predict the overall direction of equilibrium in your equation and justify your answer. (c) Calculate the pK, values for the conjugate bases of the acids in your equation. NH t H20 H30® CHy Cita OH +Ho 1300 + CHzchb0s pka =15:9 + NH3 pkw =9.24The following scenes represent three weak acids HA(where AX, Y, or Z) dissolved in water (H₂O is not shown):(a) Rank the acids in order of increasing Kₐ. (b) Rank the acidsin order of increasing pKₐ. (c) Rank the conjugate bases in orderof increasing pK(b). (d) What is the percent dissociation of HX?(e) If equimolar amounts of the sodium salts of the acids (NaX,NaY, and NaZ) were dissolved in water, which solution wouldhave the highest pOH? The lowest pH?Consider the following bases: A Which of the following statements is true? (i) The ions increase in basicity as follows: A < B < C, with C being the strongest base. (ii) The conjugate acid of C would have the highest pKa of the conjugate acids of the three bases. (iii) A is the best electron donor. O ii only O i only O two of i, ii and i O i only O None of i, ii and iii