Calculate the pH at 25 °C of a 0.32M solution of potasslum acetate (KCH,CO,). Note that acetic acid (HCH,CO,) Is a weak acid with a p K, of 4.76. Round your answer to 1 decimal place. pH =
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Q: The acid dissociation constant K, of acetic acid (HCH,CO,) is 1.8 x 10°. -5 Calculate the pH of a…
A: Since acetic acid is weak monoprotic acid. Hence it will dissociate partially as per the reaction…
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A: Given: Concentration of HCN = 3.6 M Ka = 6.2×10-10
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A: As the pH of Na2CO3 is 11.0 which means that it is basic in nature.
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A: GivenpH = 2.77pH = -logH+2.77 = -log H+H+ = 0.00169 M[H+] = 1.7 * 10-3 M
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Q: The acid dissociation constant K, of acetic acid (HCH, CO,) is 1.8× 10¯³. a Calculate the pH of a…
A: Given Ka = 1.8*10-5 [Acid] = 0.47 M To find pH the formula used pH = pKa + log[Conjugate…
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A: Given Ka for H2CO3 = 4.5 × 10-7 initial Concentration = 0.41 M
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Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10 1". а -10 Calculate the pH…
A: In this question, we want to determine the pH of the Solution. You can see details Solution below.…
Q: The acid dissociation constant K, of acetic acid (HCH3CO,) is 1.8 x 10. Calculate the pH of a 0.52M…
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Q: What is the pH of a 0.248 M aqueous solution of potasslum acetate, KCH,CO0 at 25 °C? (K, for CH,COOH…
A: 1.) Potassium acetate is a salt of conjugate base of acetic acid. So we would draw ICE table and use…
Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 × 10 '. Calculate the pH of…
A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 x 10 -10 Calculate the pH of a…
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- For CO2 in the atmosphere at 25 degrees C, kH = 3.4 x 10-2 mol L-1 atm-1 and the partial pressure of CO2 is .000405 atm: Calculate the concentration of dissolved H2CO3 (aq) air-saturated rainwater. Determine the pH expected for rainwater on the basis of the first dissociation constant of the carbonic acid, H2CO3 (aq), from the dissolved CO2. The pKa values of carbonic acid are pKa1 = 6.35 and pKa2 = 10.33 at 25 C.You are given a 27 % (w/v) solution of psicose. Molar mass: psicose (C6H12O6) = 180.156 g/mol. You dissolve 6.31 g of potassium formate in 250 mL of 0.25 M formic acid (HCOOH). This solution was then made up to a total volume of 500 mL with distilled water. Potassium formate (KHCO2): molar mass = 84.12 g/mol Calculate the pH of this solution given the pKa of formic acid = 3.77.Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.
- The pH of a saturated soloution of magnesium hydroxide, Mg(OH)2, (milk of magnesia) was found to be (1.080x10^1). From this, find the Ksp for magnesium hydroxide. Express your answer to three significant figures. Note: Your answer is assumed to be reduced to the highest power possible.Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.The pH of a saturated soloution of calcium hydroxide, Ca(OH)2, (lime water) was found to be (1.241x10^1). From this, find the Ksp for calcium hydroxide. Express your answer to three significant figures. Note: Your answer is assumed to be reduced to the highest power possible.
- The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?(a) Define and write the expression of Kw for the dissociation of water (H2O). Kw is the ________________ _____________ of ______________ (b) Calculate the pH of 0.1mol dm-3 potassium hydroxide (KOH(aq)) pH = C) Explain briefly the effect of temperature on Kw.134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence point
- Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of H2CO3 (aq) acid are 6.37 and 10.32, respectively.Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1=1x 10^3 and Ka2=1.2 x 10^(-2) .The initial concentration of sulphuric acid is given as 0.040M.Write the dissociation reactions. Calculate the concentration of [HSO4^- ] and [SO4^(2-)]. Calculate the pH of the acid solution. Write a discussion on the behaviour of polyprotic acids. (50 -100 words) Given: Ion product constant for water, Kw=1 x 10 ^(-14)Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example: CH3COO- + H2O ⇌ CH3COOH + OH- knowing that the initial concentration of the salt is 1.95 M and the acid dissociation constant, Ka , is 1.21e-7.