3. Determine the equilibrium pH of a solution made by adding HC1 (strong acid dissociate completely) to water to give a concentration of 0.01M at 25° C. Ignore activity corrections. K₁ =10-¹4 and K₁ =1000 at 25° C. W
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- Why is H3O=[OH- ]=1.0 x 10-2 M not feasible in water? What would happen if we tried to make such a solution by mixing 1.0 x 10-2 molL of KOH with 1.0 x 10-2 molLHCl?What is the pH of a saturated solution of Al(OH)3 at 25 oC, given that Ksp= 6.42 x 10-24 at this temperature? Report your answer with one decimals. Enter numbers only; do not enter units.You mix 50.0 mL of 0.250 M CH3COOH with 1.00 mL of 0.500 M NaOH. Calculate the pH of the mixture. The total volume is 51.0 mL. Use two stages method to solve this problem (I. stoichiometric reaction between acid and base, II. Acid-Base Equilibrium, ICE). Ka of CH3COOH = 1.8 x 10-5.
- The acid-dissociation constants of phosphoric acid (H3PO4) at 25 degrees Celsius are Ka1 = 7.510-3, Ka2 =6.2 10-8, and Ka3 =4.210-13. What is the PH of a 2.5M aqueous solution of phosphoric acid?1. An instrument used to measure the acidity or alkalinity of a solution. 2. Chemicals of high purity which are used to standardize a solution 3. Used as standard but have a tendency to lose water from crystallization.How to answer for Ka/ Kb and calculated pH of a solution? I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Ex. Solution 1: 30.0 mL 0.10 M CH3COOHSolution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COOSolution 3: 30.0 mL 0.10 M NH3Solution 4: 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl Sol 1,2 used methyl orange as indicatorSol 3,4 used phenolphthalein as indicator Solution w/ measured pH Ka/Kb Calculated pH 1 a 1.0 M HCl (2.01pH) b 1.0 M NaOH (3.98pH) c Control (2.91pH) 2 a 1.0 M HCl (4.73) b 1.0 M NaOH (4.82) c Control (4.76) 3. a 1.0 M HCl (10.09) b 1.0 M NaOH (11.98) c Control (11.11) 4. a 1.0 M HCl (9.13) b 1.0 M NaOH (9.38) c Control (9.30)
- At 25oC, a 100mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of the solution is 1.05g/cm3. If this solution is diluted further to form 700mL, what will be the A) [OH-], B) pH and C) % dissociation of the resulting acetic acid solution? CH3COOH -> H+ + CH3COO- (Kb = 5.56x10-10)What is the pH and fraction of association of a 0.100 M solution of a weak base with Kb = 1.00 X 10-5?Upon the addition of 30.00 mL of 0.350 M HCl to a 80.00-mL of the weak base amine (Kb = 4.95 x 10-10) whose concentration is 0.530M, the resulting pH is then equal to 5.20. True or False?
- ICE tables for 0.10 M HC2H3O 2 + 0.010 M + 0.0010 M. (ph for 0.10 M is 3.3. pH for 0.010 M is 3.7, ph for 0.0010 M is 4.4) HA(aq)<=> H+(aq) + A-(aq) Only typed solutionFull acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.Explain why the pH of mixture C is the same as the pH of mixture A C) Mixture made by mixing equal volumes of 0.2 mol L–1 HCl and 0.2 mol L–1 NaCl Conductivity (mA) 340 PH 1 A 0.1 mol L–1 HCl 260 1