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25 mL of 0.100 M AgNO3 are mixed with 35 mL of 0.0500 M K2CrO4.
(a) Calculate the concentrations of each species at equilibrium.
(b) Is the precipitation of silver quantitative (>99.9%)?
The ksp of Ag2CrO4 is 1.12*10^-12
If 6.06 L of O2 gas is collected over water at 250C (vapor pressure = 23.8 torr) and a barometric pressure of 702 torr, what is the mass of H2O2 (MM = 34.02 g/mole) decomposed?
A buffered solution is made by adding 50.9 g NH4Cl to 1.00 L of a 0.75 M solution of NH3. Calculate the pH of the final solution. (Assume no volume change.)
what are the possible sources of error when finding the density of a liquid and of a solid? what can be done to avoid these errors?
At what pH will an aqueous solution of 0.210 M Mn2+ begin to precipitate as Mn(OH)2 at 25 °C? The Ksp for Mn(OH)2 is 1.9 x 10-13
When a chiral carbon contains a hydrogen, you should not show the hydrogen, but you must use either a wedge or dashed bond and 2 sticks to establish stereochemistry.
what is the concentration of sodium ions in the resulting solution?
Ddetermines how many tablets should be given to her if there are five tablets in stock.
If a cell is in a resting state, which of the following is NOT true: a. cell needs little energy b. high ATP, low ADP levels
calculate the external pressure that must be applied to seawater, 1.14 M total ion concentration at 10 degrees celcius if the maximum concentration allowed in the product water is 166 mg/L
Calculate the pH at the equivalence point in the titration of 25.00 mL of 0.120 M chloropropanoic acid (Ka = 7.8 x 10-5)
Solid copper (II) hydroxide from copper nitrate. First, add 30 mL of 3.0M sodium hydroxide to the solution in the Erlenmeyer Flask.Take a stirring rod and place the end about 1 cm into the solution; then tough the end to a 2 cm piece of red litmus..
An ionic compound forms when aluminum (Z = 13) reacts with iodine (Z = 53). If a sample of the compound contains 1.23 x 1019 aluminum ions.
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