A 55.00 mL sample of bottled water is titrated with 0.00033000 M silver nitrate to determine...
A 55.00 mL sample of bottled water is titrated with 0.00033000 M silver nitrate to determine the concentration of dissolved chloride. The end point is determined electrochemically. At the endpoint it was determined that 17.26 mL of titrant was used. What is the molarity of chloride in the original sample?
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A 55.00 mL sample of bottled water is titrated with 0.00033000 M
silver nitrate to determine...
What is the molar concentration of a silver nitrate titrant if 42.51 mL of the titrant...
What is the molar concentration of a silver nitrate titrant if 42.51 mL of the titrant are required to reach the endpoint when testing 0.524 g of sodium chloride standard (58.443 g/mol)? AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.026 M HCl, and...
A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.026 M HCl, and the endpoint is reached after 35.9 mL of titrant are dispensed. Based on this data, what is the concentration of the hydroxide ion?
1. A 10.00 mL aliquot of 0.010 M CaCO3 is titrated with 18.22 mL of EDTA...
1. A 10.00 mL aliquot of 0.010 M CaCO3 is titrated with 18.22 mL of EDTA solution. What is the EDTA molarity? 2. A 250.0 mL water sample requires 30.85 mL of the EDTA solution from question 1 to reach the calmagite endpoint. What was the molarity of the hard metal ions in the water sample? 3. If the metal ions in the water sample of question 2 are assumed to be Ca2+ from CaCO3, express the concentration in ppm...
1) A 25.00 mL sample of HBr is titrated with a 0.150 M standardized sodium hydroxide...
1) A 25.00 mL sample of HBr is titrated with a 0.150 M standardized sodium hydroxide solution. The endpoint was reached when 18.80 mL of titrant had been added. Calculate the molar concentration of the HBr.
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with...
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.455 g of precipitate, what is the molarity of silver ion in the original solution? M
A 200.0 mL sample of water was titrated with 0.00355 M K2Cr2O7 to determine chemical oxygen...
A 200.0 mL sample of water was titrated with 0.00355 M K2Cr2O7 to determine chemical oxygen demand. If it required 26.3 mL of potassium dichromate to reach the end point, what is the COD of water in mg O2/L?
The silver nitrate in 20.00 mL of a certain solution was allowed to react with sodium...
The silver nitrate in 20.00 mL of a certain solution was allowed to react with sodium chloride according to the following equation AgNO3 + NaCl yields AgCl + NaNO3 The AgCl was collected, dried and weighted to .2867g AgCl What was the molarity of the original silver nitrate solution?
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chlori
suppose an EPA chemist tests a 200.mL sample of groundwater known to be contaminated with tin(II) chloride, which would react with silver nitrate solution like this:SnCl2(aq) + 2AgNO3(aq) → 2AgCl(s) + SnNO32(aq)The chemist adds 22.0mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 7.6mg of silver chloride.Calculate the concentration of tin(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits.
To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in...
To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in a flask and titrated with a 0.1433 M solution of cesium hydroxide. A volume of 20.29 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of sulfuric acid in the original sample. A student has 530.0 mL of a 0.1474 M aqueous solution of MnSO4 to use in an experiment. He accidentally leaves the container uncovered and comes back the next week...
A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.026 M HCl, and the endpoint is reached after 35.9 mL of titrant are dispensed. Based on this data, what is the concentration of the hydroxide ion?
1) A 25.00 mL sample of HBr is titrated with a 0.150 M standardized sodium hydroxide solution. The endpoint was reached when 18.80 mL of titrant had been added. Calculate the molar concentration of the HBr.
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.455 g of precipitate, what is the molarity of silver ion in the original solution? M
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