A 0.051 M solution of a weak acid has a pH of 2.09. Calculate the acid ionization constant (Ka) of the acid. Express your answer to 2 significant figures. Ka
Q: 5) a) Calculate the pH of 5 liters, 1.00 M HA weak acid solution. (Ka= 6.8 x 10*) Calculate the…
A: 5 a. Given: Ka = 6.8×10-4 Initial concentration of HA = 1.0 M
Q: Calculate the pH of a 0.10 M solution of hypochiorous acid, HOCl. Ka of HOCI is 3.5 x 10^-8 at 25…
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Q: Determine the pH of a 0.62 M NH4NO3 solution at 25°C. The Kb for NH3 is 1.8 × 10-5. Express your…
A: NH4NO3 is a salt of strong acid and weak base. Given Kb of ammonia is 1.8×10-5 and concentration of…
Q: Calculate the pH of a 0.27 M solution of HCO2H (formic acid, Ka = 1.8 x 10–4).
A: PH = - log [H +] Formic acid weak acid Ka =dissociation constant
Q: 1. (a) calculate the hydrogen ion concentration in a 0.200 M solution of propanoic acid. The acid…
A: Degree of dissociation of a weak acid in a solution (α) = (Ka/C)1/2 [H+] = (Ka x C)1/2 % Ionization…
Q: The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization…
A: Given : We have to calculate the ionization constant.
Q: When answering this problem, report the answer with the appropriate number of significant figures.…
A: When a solution is diluted by adding water, concentration changes.
Q: 2.2 6. (1) Define pH in words. The strong acid HCl has a pH value of 1, use the following equation…
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Q: A chemist dissolves 213. mg of pure barium hydroxide in enough water to make up 130. mL of solution.…
A: pH of a solution is defined as the negative log of the hydrogen ion concentration. pOH of a solution…
Q: Compounds containing nitrogen are often weak bases. One example is aminoethanol, which has the…
A: The relation between pH and pOH: pH= 14 - pOH
Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…
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Q: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka)…
A: Given:
Q: Given that Ka for HCN is 6.2×10−10, calculate Kb for CN-. Express your answer to two significant…
A: 1- First question, Calculate the value of Kb for weak base CN- ion : We know that, Kb × Ka = Kw Kb…
Q: Be sure to answer all parts. The pH of a 0.064 M weak monoprotic acid is 3.09. Calculate the Ka of…
A: Given,The pH of a 0.064 M weak monoprotic acid is 3.09
Q: A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of…
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Q: Classify each acid as strong or weak. If the acid is weak, write an expression for the acid…
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Q: Calculate the pH of the following solutions. Give your answers to two significant figures. (a) 0.021…
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Q: Identify if the statement is true or false. Provide calculations to support your answer. The…
A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…
Q: A 0.125 M weak acid (HA) solution has a pH of 2.25. Find the acid ionization constant, Ka-
A: Given that : Initial concentration of weak acid = 0.125 M pH = 2.25 The pH can be given by : pH =…
Q: The ionization constant of water at a certain temperature is 1.7 x 10-14. Calculate the pH of water…
A: given, the ionisation constant of water, Kw = 1.7×10-14 using, Kw = [H+][OH-]
Q: Calculate the pH of the following solutions. Give your answers to two significant figures. (a) 0.021…
A: pH is defined as the negative logarithm of Hyrnium ion concentration pH = - log[H3O+] or pH…
Q: When a 0.061M aqueous solution of a certain acid is prepared, the acid is 2.1% dissociated.…
A: For a weak acid - WA ⇔ W+ + A- The reactants and products are in equilibrium. Since…
Q: Maleic acid (H2C4H2O4) is a diprotic acid with ?a1=1.20×10−3 and ?a2=5.37×10−7. Determine the pH of…
A: 1- First we will determine the H+ ion concentration : Most H+ ion comes from first dissociation.…
Q: The acid dissociation constant K, of boric acid (H,BO3) is 5.8 × 10 Calculate the pH of a 2.5M…
A: Give, the dissociation constant (Ka) of boric acid = 5.8×10-10 We have to calculate the pH of a 2.5…
Q: Since the pH of 0.1 M acetic acid solution is measured as 2.88, the Ka value of acetic acid…
A: The degree of ionization has to be calculated, Given, The pH of the solution is 2.88. We know that…
Q: Construct the expression for Ka for the weak acid, CH-COOH. CH.COOH(aq) + H₂O(l) = H₂O (aq) + CH.COO…
A: Ka is the ratio of the equilibrium concentrations of product over equilibrium concentrations of…
Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…
A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…
Q: The pH of a 0.70 M solution of propanoic acid (HC,H;0,) is measured to be 2.51. Calculate the acid…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka)…
A: The concentration of HA = 0.115 M pH = 3.29 pH = 3.29H3O+ =10-pH=10-3.29=0.000513 M
Q: Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation…
A: Given data is as follows: The mass of aspirin = 2.00 g The volume of water = 0.600 L The pH of the…
Q: A 2.76 M solution of monoprotic acid HA has a pH of 1.216 at 25 °C. Calculate the acid-ionization…
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Q: A0.9000M solution of hydrosulfuric acid is only partially ionized. Using measurements, the resulting…
A: The dissociation reaction for hydrosulfuric acid (H2S) can be given as- H2S(aq)↔H+(aq)+HS-(aq) The…
Q: Without using a calculator, determine the pH and pOH of each solution. Rank the solutions from most…
A: pH of the solution is equal to the negative logarithm of hydronium ion concentration while pOH is…
Q: Formic acid owes its name to the fact that some ant (fourmi) species have specialised soldiers that…
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Q: Calculate the pH of an aqueous solution that is 0.35 M NH3 and 0.15 M NHẠNO3 given that the K of NH3…
A: Given solution which have NH3 ( a weak base ) and NH4NO3 ( conjugate salt of NH3) , would form a…
Q: A 0.015 M solution of hydrogen cyanate (HOCN) has a pH of 2.67. Calculate the hydrogen cyanate…
A: Calculate the concentration of hydronium ion:
Q: propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M
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Q: The acid dissociation constant Ka of carbonic acid (H2CO3) is 4.5x10^−7. Calculate the pH of a 4.5M…
A: Given :- Concentration of H2CO3 solution = 4.5 M Ka for H2CO3 = 4.5 × 10-7 To calculate :- pH of…
Q: A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of…
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Q: Enough water is added to 0.35g of benzoic acid to make 1000 mL of a solution. What is the pH?…
A: Given: Mass of benzoic acid=0.35 g Volume of solution=1000 mL =1 L Ionization constant for benzoic…
Q: What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…
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Q: The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar…
A: Ionization of acetic acid(CH3COOH): CH3COOH(aq) ⇌…
Q: A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar…
A: Given : Acetic acid solution (i.e vinegar) with pH = 2.90 Ka of acid = 1.8 X 10-5 The dissociation…
Q: The weak acid HCN has Ka= 6.2 x10-10. Determine the pH of a 4.597 M solution of HCN.
A: Given: weak acid HCN with Ka= 6.2 x10-10 To find: pH of a 4.597 M solution of HCN.
Q: Calculate the molar H3O+ ion concentration of a solution that has a pH of 4.75 Express your answer…
A: pH of the solution is the negative logarithmic of Hydrogen ion concentration .From pH we can…
Q: If you have a 0.1650 M solution of a base is 6.1% ionized, then calculate the base ionization…
A: A base is a compound that accepts H+ ion (proton). Bases dissociate in water to release OH- ions…
Q: Sulfuric acid (H2SO4) has two acidic protons with the following ionization constants: Ka1 is…
A: As we know, Strong acid dissociates completely and releases [H+] ion. So, we can calculate directly…
Q: Calculate the pH of a 0.10M weak acid, HA, whose Ka is 1.8 X 10
A: Given that: Concentration of weak acid,(HA) = 0.10M Ka = 1.8×10-5 Weak acid partially dissociates…
Q: What will be the pH of a solution of a weak acid (HB), of concentration 0.15 M (Ka = 1.8x10-5
A:
Q: Calculate the pH, when the following solutions are added to 100. mL 0.10 M HClO solution: The Ka of…
A: Given :- Molarity of HClO solution = 0.10 M = 0.10 mol/L Ka of HClO = 3.0 x 10-8…
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- Equimolar solutions of HF, HCOOH and HCN at 298 K have the values of Ka as 6.8×10^-4, 1.8×10^-4 and 4.8×10^-9 respectively. What will be the order of their acidic strength?Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Define the term" WEAK ACID"Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5.
- For H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by systematic methodA solution of nitric acid, HNO2, at a concentration of 0.495M was found to be 1.83 = pH. A. Calculate the concentration [H3O(aq)+] And the ionization percentage of the nitric acid. ShowCalculations. B. Write the expression for the existing equilibrium in the solution and calculate the value of Ka ofNitric acid. Show calculations. C. Calculate the pH of the resulting solution by adding 0.1 g of NaNO2 to750 ml of HNO2 solution 0.0125M. Show calculations. D. Schematically plot the titration curve of 20.0 mL HNO2 0.0125MWhich is purged with NaOH 0.0125M while specifying the names of the axes. Marked on topThe curve the buffer area and the equivalent point. Detail the calculationsWhich led to the drawing of the curve.calculate the PH of 1.5 M solution of hydroxylamine at 25 degrees C with a Kb = 9.1 times 10^-9
- Calculate the pH and percent ionization of a .25 M solution of weak base pyridine. Given Kb = 1.7 * 10^-9 (show the equation for the proton trasfer equlibrium with H2O)Give a clear handwritten answer... An aqueous solution of base has a concentration of 0.156 M (@ 25 °C). The conjugate acid of the base is known to have a Ka value of 6.32 x 10-6. What is the pH of the solution?The pH at 25 °C of an aqueous solution of the sodium salt of α-naphthol (NaC10H7O) is 11.23. Calculate the concentration of C10H7O- in this solution, in moles per liter. Ka for HC10H7O is equal to 4.6×10-10.
- Phenolphthalein has a pKa of 9.7. It is colorless in its acid form and pink in its basic form. For each of the values of pH, calculate [In-]>[HIn] and predict the color of a phenolphthalein solution. a. pH = 2.0 b. pH = 5.0 c. pH = 8.0 d. pH = 11.0Like any equilibrium constant, Kᵥᵥ changes with tempera-ture. (a) Given that autoionization is endothermic, how does Kᵥᵥ change with rising T? Explain with a reaction that includes heatas reactant or product. (b) In many medical applications, the value of Kᵥᵥ at 37°C (body temperature) may be more appropri-ate than the value at 25°C, 1.0X10⁻¹⁴. The pH of pure water at 37°C is 6.80. Calculate Kᵥᵥ, pOH, and [OH] at this temperature.Suppose a weak acid has Ka = 4.0 x 10^-9. which is equivalent to Kb? and why??