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4.62 (a) Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water to form exactly 550 mL of solution. (b) How many moles of KBr are present in 150 mL of a 0.275 M solution? (c) How many milliliters of 6.1 M HCl solution are needed to obtain 0.100 mol of HCl?
how many grams of silver nitrate are present when 8.50 g of silver are in a sample?
a saturated solution of potassium chlorate is dissolved in 100g of water. If the saturated solution is cooled from 90oC to 60oC, how many grams of precipitate will be formed?
170mL of an HCl solution with pH of 2.80 is added to 200mL of an HNO3 solution. The resulting pH is 1.40. What was the pH of the original HNO3 solution
The mixture is diluted with deionized water to the mark and shaken vigorously. What mass of AgBr would precipitate from this mixture?
The reaction, seen below, is carried out in a constant-volume flask. Initially only dimethyl ether is present and the pressure is 0.350 atm. What is the pressure of the system after 8.0 minutes? Assume ideal behavior.
Consider the titration of 50.0 mL of 0.20 M NH 3 (K b =1.8×10 ?5 ) with 0.20 M HNO 3 . Calculate the pH after addition of 50.0 mL of the titrant.
calculate the final temperature of the water after all the ice melts. heat capacity of H2O: 37.7 J/mol*k heat capacity of H2O l: 75.3 J/mol*k enthalpy of fusion of H2O: 6.01 kJ/mol
Silver consists of two major isotopes with the following percent abundances and atomic masses: 107Ag (51.84% and 106.90509 amu) and 109Ag (48.16% and 108.90476 amu). Calculate the average atomic mass of silver to five significant digits.
Match the detector or detectors that can be used in gas chromatography for the detection of the following list of analytes by dragging the detector into the box to the left of the analyte.
Consider a solution resulting from the mixing of precisely 50.0 mL of 2.0 M NaOH with 50.0 mL of 2.0 M HCl. Will the mixture be corrosive and damage the skin or will it become a salt solution that is safe enough to drain down the sink.
an acetic acid solution of 2.87 pH is titrated with 1.5 mL of bromocresol green. When the color changes to light green
Other than S=C=S; can I have S triple bonded to C single bonded to S? Wouldn't there be three electrons left on the triple bonded S; it would be sharing three when it started with six I don't understand? Help please.
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