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- You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.DETERMINATION OF TOTAL AMOUNT OF ACID IN WINE C4H6O6 + 2 NaOH → (C4H4O6) Na2 + 2 H2O A sample of 10 mL of wine was taken and the volume was completed to 50 mL by adding pure water. This solution was titrated with 0.1 M NaOH and 24 mL of NaOH was spent. According to this Calculate the amount of tartaric acid in wine as g / L.A 2.00 mL sample of serum is analyzed for protein by the modified Kjeldahl method. The sample is digested and the resulting ammonia is distilled into a boric acid solution, consuming 15.0 mL of standard HCl to titrate the ammonium borate. HCl is standardized by treating 0.330 g of pure (NH₄)₂SO₄ in the same way. If 33.3 mL of acid is consumed in the standardization titration, what is the serum protein concentration in g% (wt/vol)?
- Q7. Karl Fisher titration is used to determine moisture content of food products according to the chemical reaction below: 2H₂O + SO₂ + 12 → H₂SO4 + 2HI (i) Name the reaction that involved. (ii) Identify the FOUR major chemical components needed in the Karl Fisher reagents. (iii) Rewrite the actual chemical reaction(s) that involved during Karl Fisher titration. (iv) Outline the function of each major chemicals in the reaction stated in answer (iii).A municipal water sample has 0.20 ppm Pb2+ by weight. The density of this sample is 1.00 g/mL. How many milligrams of Pb2+ is in 1 L of this water sample? 2 x 10-4 mg 2 x 10-1 mg 2 x 10-7 mg 2 x 10-10 mg What is the concentration of Cr3+ in a saturated solution of chromium (III) hydroxide (Ksp = 6.3 x 10-31)? You may ignore activity effects. 6.3 x 10-31 M 7.9 x 10-16 M 8.5 x 10-11 M 1.2 x 10-8 MA chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 42. mg of oxalic acid (H,C,0.), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 46.1 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. |x10 M
- Human blood has a pH of approximately 7.4 due to the carbonic acid/bicarbonate ion (H2CO3/HCO3−) buffer system. Any pH changes below 6.8 or above 7.8 can lead to death! Carbonic acid dissociates to form water and carbon dioxide in the equilibrium shown below. This process is crucial in respiration. H2CO3 (aq) ⇋ CO2 (g) + H2O pKa1 = 2.77 Carbonic acid dissociates in water to form the bicarbonate ion and the hydroxonium ion by the following equilibrium reaction:H2CO3 (aq) + H2O ⇋ H3O(aq)+ + HCO3− pKa2 = 3.70 (i) If there is a 25% increase in carbonic acid levels as per pKa1, explain how the body would deal with this change.Q5: A sample of 0.676g of an unknown compound containing barium ions (Ba+) is dissolved in water and treated with an excess of NazSO. If the mass of BasO, precipitate formed is 0.4105g. What is the percent by mass of Ba in the original unknown compound? Note: Mwt. of Ba =32, Mwt. of BaSo4 =233, Mwt. of Na2SO4=142A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate- buffered solution. The reactions that occur are I2 + 2e- = 2I N2H4 .H2SO4 → N2 + SO4 2- + 6H+ + 4e- What is the molarity of a solution of hydrazine sulfate when 27.29 mL of 0.100 N iodine is required to titrate 25.00 mL of the hydrazine sulfate to the equivalence point?
- 2. Titrate 1.2035g of solid KHP (KCH;O4) requires 23.89 mL of an unknown NaOH solution to reach the equivalence point. What's the molarity of this unknown NaOH solution? Show your work.When the reversible reaction HC2H;O2 (aq) E> H(aq) + C2H3O2 (aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of NaOH (aq) to the reaction mixture? a) pH will not change because NaOH is not a part of the reaction equation. b) pH will not change because acetic acid and NaOH form a buffer. c) pH will increase because NaOH will completely neutralize acetic acid. d) pH will decrease because NaOH will completely neutralize acetic acid. In the reversible reaction A (aq) + B(aq) E > C(aq), reactant A is very expensive. What are two ways to get it to react as fully as possible to form as much C as possible? a) remove C as it forms, and use an excess of A b) add another reactant that will form a precipitate with B c) remove C as it forms, and use an excess of B d) add another reactant that will form a precipitate with AWhat mass of CO2 is formed if 100 g of CaCL2 is also formed in the reaction below CaCO3 + 2 HCL——> CaCL2+ H2O + CO2