Determine the amount of KCl in the first sample, as 25 mL of the sample taken...
Determine the amount of KCl in the first sample, as 25 mL of the sample taken from 250 mL of KCl solution is titrated with 34 mL of 0.1050 M AgNO3 solution. (Ma K=39 g/mol, Ma Cl =35.5 g/mol)
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Determine the amount of KCl in the first sample, as 25 mL of the
sample taken...
A mixture only contains KCl and NaBr is analysed using Mohr method. A sample of this...
A mixture only contains KCl and NaBr is analysed using Mohr method. A sample of this mixture weighing 0.3172 g is dissolved in 50.00 mL distilled water and titrated to an end-point 36.85 mL of 0.1120 M AgNO3 solution. The blank titration required 0.71 mL to reach the same end-point. Calculate the percentage (w/w) of KCl and NaBr each in the same sample. [RMM: KCl = 74.6, NaBr = 102.9]
Given 25 ml of a KCl solution with a concentration of 0.38 M and 18 ml...
Given 25 ml of a KCl solution with a concentration of 0.38 M and 18 ml of a solution of CaCl2 with a concentration of 0.19 M, what amount of each solution you should use to make 40 ml of solution with [Cl-]=0.30 M ?
33) If 100. mL of water is added to 25 mL of 5.0 M NaCl solution,...
33) If 100. mL of water is added to 25 mL of 5.0 M NaCl solution, what is the final concentration? 34) Calculate the volume of 0.123 M AgNO3(aq) needed to form 0.657 g of Ag2SO4(s) according to the chemical equation: 2AgNO3(aq) + H2SO4(aq) -----> Ag2SO4(s) + 2H20(1). 35) Calculate the concentration of a KCl solution prepared by adding 200. mL of water to 100 mL of 12% KCl solution.
A 0.7498-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting...
A 0.7498-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 48.85 mL of a 0.2298 M AgNO3 solution. This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.1165 M KSCN and required 20.82 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45...
Not a real experiment, just a homework question In order to test the concentration of chlorine ions, Cl - (aq) in a water reservoir, a sample of 300 ml was taken from a water reservoir to the laborato...
Not a real experiment, just a homework question In order to test the concentration of chlorine ions, Cl - (aq) in a water reservoir, a sample of 300 ml was taken from a water reservoir to the laboratory and a number of experiments were performed. In the first stage, the sample was divided into two cups. A 100 mL solution was prepared in the first glass, and in the second glass 200 ml Several experiments were performed. First cup -...
Question A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution...
Question
A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion. Ag+...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this...
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion....
KOH (concentration = 0.2205 M) is used in a titration to determine the amount of acetic...
KOH (concentration = 0.2205 M) is used in a titration to determine the amount of acetic acid (CH3COOH) in vinegar! 50 mL of vinegar was diluted to 500 mL in a volumetric flask. 25 mL of the diluted vinegar solution was titrated five times with the KOH. The concentration of acetic acid in the DILUTED vinegar sample is 0.2171 M Calculate the concentration of acetic acid in the ORIGINAL vinegar solution Give your answer in g/L MM CH3COOH = 60.05...
PLEASE SHOW WORK The standard enthalpy of solution for KCl(s) dissolving in water to form 1...
PLEASE SHOW WORK
The standard enthalpy of solution for KCl(s) dissolving in water to form 1 m solution of aqueous K^+ and Cl^- ions, delta H^0 _soln = +17.2 kJ/mol. Using a coffee calorimeter, 0.15 moles of KCl(s) were dissolved in 150 mL of water. The initial water temperature was 25 C. What would be the final temperature? A 4C B 21 C C 25 C D 29 C E 42.2 C
33) If 100. mL of water is added to 25 mL of 5.0 M NaCl solution, what is the final concentration? 34) Calculate the volume of 0.123 M AgNO3(aq) needed to form 0.657 g of Ag2SO4(s) according to the chemical equation: 2AgNO3(aq) + H2SO4(aq) -----> Ag2SO4(s) + 2H20(1). 35) Calculate the concentration of a KCl solution prepared by adding 200. mL of water to 100 mL of 12% KCl solution.
Question
A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion. Ag+...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion....
PLEASE SHOW WORK
The standard enthalpy of solution for KCl(s) dissolving in water to form 1 m solution of aqueous K^+ and Cl^- ions, delta H^0 _soln = +17.2 kJ/mol. Using a coffee calorimeter, 0.15 moles of KCl(s) were dissolved in 150 mL of water. The initial water temperature was 25 C. What would be the final temperature? A 4C B 21 C C 25 C D 29 C E 42.2 C
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