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Q: Calculate the pH of a 0.75 mol L─3 solution of ethanoic acid at 298 K. Given Ka = 1.7 × 10─5
A: Welcome to bartleby ! We have to calculate pH .
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Q: 10.06 cm3 of the stock 0.100 mol dm-3 solution of NaOH was required to fully neutralise 49.5 mg of a…
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Q: What is the pH of a 1.63 M solution of XOH, a weak monobasic compound (Kb = 1.7 x 10^-9)?
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Q: Calculate pH and pOH of the: 0.5M aniline (C6H5NH2) solution (Kb= 3.8 x 10-10)
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Q: The acid dissociation constant for acetic acid (HC2H3O2, commonly abbreviated HAc) is 1.8 x 10-5.…
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Q: What is the pH of a 0.420 M solution of C5H,NHB (Kb of C5H,N is 1.7 × 10-9)?
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Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3 with deonised water.
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- Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa = 4.76) of (a) 2:1; (b) 1:3; (c) 5:1; (d) 1:1; (e) 1:10(a) Write a balanced equation representing the reaction of the acid, H2PO4- with the base, water. (b) Write the expression for Ka of H2PO4- in terms of concentrations of relevant species.8. (a) How many grams of ammonium bromide would have to be added to exactly 500 cm³ of 0.10 M NH3 solution to have a pH of 8.5. I (a) How many grams of sodium acetate must be added to 0.100 dm³ of 0.2 M acetic acid to give a pH of 4.0?
- What is the pH of a solution that is a prepared by dissolving 4.90 g of (NH4)2SO4 ( K₁ (NH4+) = 5.70 × 10-¹0) in water, adding 150.0 mL of 0.1263 M NaOH, and diluting to 900.0 mL? pH = b0.124 M in piperidine and 0.054 M in its chloride salt ( Ka (C5H₁1NH+) = 7.50 × 10−¹² )? -12 pH = C prepared by dissolving 2.12 g of aniline (93.13 g/mol, Ką (anilinium ion) = 2.51 × 10−5) in 100. mL of 0.0330 M HCl and diluting to 500.0 mL? pH =The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.10.06 cm³ of the stock 0.100 mol dm-3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid.
- 6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.Calculate the pH of a 0.05 mol dm-3 CH3COOH solution; the dissociation constant Ka for CH3COOH is 1.72 x 10-5 mol dm^-3 .
- Acetic acid (CH3COOH, abbrev. HA) is a very common weak acid with pKA = 4.75 (at 25oC and low ionic strength). Calculate pH of the diluted solution of acetic acid with concentration c = 0.05 mol dm-3.Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O (m = NH4*(aq) + OH-(aq) At 25°C, Kb, is 1.8 × 10-5 (7) Calculate the pH of a mixture of 0.192 mol NH3 and 0.116 mol NH4C1 diluted to 400.0 mL with distilled water.(iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml samples of distilled water. Calculate [H30*] and the pH for each of the resulting solutions and comment on the relationship between [MgCl2] and pH.