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A 25.0 mL solution of 0.20 M Ethylamine (CH3CH2NH2, Kb = 5.6 x 10-4) was
titrated with 0.15 M HCl.
CH3CH2NH2 (aq) + HCl(aq)→ CH3CH2NH3+(aq) + Cl−(aq)
a. What volume (mL) of HCl must be used to reach the equivalence point?
b. What is the pH at the equivalence point?
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- A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid. Cr(NH3)xCl3(aq) + x HCl(aq) x NH4+(aq) + Cr3+(aq) + (x + 3) Cl(aq) Assume that 24.26 mL of 1.500 M HCl is used to titrate 1.580 g of Cr(NH3)xCl3. What is the value of x?
- A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.You have been provided with a 35.7 mL sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 1.75 M nitric acid (HNO3), and find that 2.37 × 10−2 L are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L−1? Report your answer to the correct number of significant figures.The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail
- A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. a) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) b) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. c) Calculate the mass percent of acetic acid, HC2H3O2(aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.What is the mass of sodium oxalate (Na2C2O4, MM = 134,00 g/mol), in mg, should be taken so that in its titration 25,00 mL of a solution of potassium permanganate (KMnO4) 0,032 mol/ L in strong acid medium? 21,4 mg 268 mg 536 mg 107 mg 134 mg
- Acetic Acid reacts with sodium hydroxide in the following fashion:CH_3COOH(aq)+NaOH(aq) > H2O(l)+NaC2H3O2(aq) If 3.60mL of vinegar needs 41.0mL of 0.150M NaOH to reach the equivalence point in a titration how many grams of acetic acid are in a 1.50 qt sample of this vinegar? Express your answer using three significant figures5.00 mL of 2.5 M NaCl(aq) is diluted with water to the calibration line in a 100.00 mL volumetric flask. What is the concentration of the new solution?The amount of ascorbic acid (vitamin C; C6H8O6) in tablets is determined by reaction with bromine and then titration of the hydrobromic acid with standard base: C6H8O6(aq) + Br2(aq) → C6H6O6(aq) + 2HBr(aq) HBr(aq) + NaOH(aq) → NaBr(aq) + H2O(l)A certain tablet is advertised as containing 500 mg of vitamin C. One tablet was dissolved in water and reacted with Br2. The solution was then titrated with 43.20 mL of 0.1350 M NaOH. Did the tablet contain the advertised quantity of vitamin C?
