Q: Calculate the pH of a 0.0158 M aqueous solution of formic acid (HCOOH, Ka = 1.8x10 4). %3D pH =
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A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid
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A: a.
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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: If 1.00 mol of HCOOH and 0.500 mol of NaHCOO are added to water and diluted to 1.00 L, calculate the…
A: Given: Moles of HCOOH = 1.00 mol Moles of NaHCOO = 0.500 mol Volume of solution = 1.00 L Acid…
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A: Ka for general acid dissociation reaction is,
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Q: Calculate the pH and percent ionization of 0.05 M acetic acid Ka = 1.8 x 10 -5. %3D
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Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00789 M…
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Q: Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…
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Q: Calculate the pH of 0.400 M solution of ascorbic acid, HC6H;O6. (Ka of ascorbic acid = 6.80 x 105)
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Q: The acid dissociation constant K of alloxanic acid (HC,H,N,05) is 2.24 x 10 a. Calculate the pH of a…
A: [HA] = 2.8 M ( concentration of alloxanic acid ) Ka = 2.24 × 10-7 pH =?
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- Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.Calculate the pH at 25 °C of a 0.23 M solution of sodium hypochlorite (NaClO). Note that hypochlorous acid (HCIO) is a weak acid with a pK, of 7.50. a Round your answer to 1 decimal place. pH = 0 ?The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10¯¹⁰. Calculate the pH of a 6.9M solution of hydrocyanic acid. Round your answer to 1 decimal place.
- Calculate the pH at 25 °C of a 0.26M solution of potassium cyanide (KCN). Note that hydrocyanic acid (HCN) is a weak acid with a pK of 9.21. Round your answer to 1 decimal place.Predict the position of equilibrium and calculate the equilibrium constant, Keq, for acid-base reactionPhosphoric acid, H3PO4(aq),H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.150 M phosphoric acid solution. pKa1= 2.16 pKa2= 7.21 pKa3= 12.32 [H3PO4]= ? M [H2PO−4]= ? M [HPO2−4]= ? M [PO3−4]= ? M [H+]= ? M [OH−]= ? M pH=
- The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10 10 Calculate the pH of a 3.0M solution of hydrocyanic acid. Round your answer to 1 decimal place. pH = 0If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula C;H,N |1.7 × 10~9 4 hydrofluoric acid HF 6.8 × 10 pyridine 10 4.9 x 10 alo 4 hydrocyanic acid НCN ethylamine C2H,NH, | 6.4 × 10 Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the sofution t will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C2H5NH3B choose one 0.1 M C5H5NHCI choose one v 0.1 М KI choose one v 0.1 M KF choose one
- Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.The acid dissociation constant Ka of boric acid (H,BO,) is 5.8 x 10 . Calculate the pH of a 3.2M solution of boric acid. Round your answer to 1 decimal place. pH =Perform the following to determine the pH of a lactic acid solution. Write the acid/base reaction between lactic acid, HC3H5O3 and water. Write an equilibrium expression for the reaction between lactic acid and water. If the Ka of lactic acid is 3.18 x 10-4, what is the pH of a 0.500 M solution of lactic acid?