Solution preparation calculators

For each of the following solutions, the number of moles of solute is given, followed hy the total volume of solution prepared. Calculate the molarity. 

Calculate the molarity of a potassium dichromate solution prepared by placing 9.67 g of K2Cr207 in a 100-mF volumetric flask, dissolving, and diluting to the calibration mark. 

Calculate the osmotic pressure at 15°C of a solution prepared by dissolving 50.0 g of sugar, C12H22O11, in enough water to form one liter of solution. 

Butyric add, HC4Ht02, is responsible for the odor of rancid butter and cheese. Its K is 1.51 X 10 5. Calculate [H+] in solutions prepared by adding enough water to the following to make 1.30 L. 

The main advantages of the method can be formulated as follows. First, hydrofluoric acid is not needed for the decomposition stage the amount of fluorine required for the raw material decomposition can be calculated and adjusted as closely as possible to the stoichiometry of the interaction. Since the leaching of the fluorinated material is performed with water, a significant fraction of the impurities are precipitated in the form of insoluble compounds that can be separated from the solution, hence the filtrated solution is essentially purified. There is no doubt that solutions prepared in this way can be of consistent concentrations of tantalum and niobium, independent of the initial raw material composition. 

Procedure. To 100 mL of the neutral sample solution (containing not more than 0.4 mg nitrite) add 2.0 mL of solution A and, after 5 minutes, 2.0 mL of solution B. The pH at this point should be about 1.5. Measure the absorbance after 10 minutes in the wavelength region of 550 nm (yellow-green filter), in a spectrophotometer against a blank solution prepared in the same manner. Calculate the concentration of the nitrite from a calibration plot prepared from a series of standard nitrite solutions. 

Reagents. Standard calcium solution. Prepare a standard solution containing 40.0 mg L 1 calcium by dissolving the calculated quantity of calcium carbonate in the minimum amount of hydrochloric acid and diluting to 1 L in a graduated flask. 

A solution prepared from Mo202L4 (concentration 2C, where L = Et2NCSe2) in 1,2-dichloroethane was mixed with the same volume of solvent. The absorbance of the solution decreased exponentially. Use the following linear equation of k2 against C to calculate the rate constants ... 

Self-Test 8.8A Calculate the molality of ZnCl2 in a solution prepared by dissolving 4.11 g of ZnCI2 in 150. g of water. 

Calculate the vapor pressure of water at 20.°C in a solution prepared by dissolving 10.00 g of the nonelectrolyte sucrose, C12H2201, in 100.0 g of water. 

Sfi.f-Test 8.1 IB Calculate the vapor pressure of ethanol in kilopascals (kPa) at 19°C for a solution prepared by dissolving 2.00 g of cinnamaldehyde, C9HkO, in 50.0 g of ethanol, C2F-I5OH. The vapor pressure of pure ethanol at that temperature is 5.3 kPa. 

Calculate the concentrations of each of the following solutions (a) the molality of chloride ions in an aqueous solution of iron(lll) chloride for which is 0.0205 (b) the molality of hydroxide ions in a solution prepared from 9.25 g of barium hydroxide dissolved in 183 g of water. (c) the molality of 12.00 M NH,(aq) with a density of... 

To determine the mass of NiCl2 6 H2 O required to prepare the solution, first calculate the number of moles of the salt required, and then use the molar mass to determine the mass in grams ... 

C03-0035. Calculate the concentration of ammonium nitrate in a solution prepared by dissolving 3.20 g of the salt in enough water to make 100. mL of solution, then diluting 5.00 mL of this solution to a volume of 25.00 mL. 

C03-0093. A student prepares a solution by dissolving 4.75 g of solid KOH in enough water to make 275 mL of solution, (a) Calculate the molarities of the major ionic species present, (b) Calculate the molarities of the major ionic species present if 25.00 mL of this solution is added to a 100-mL volumetric flask, and water is added to the mark, (c) Draw molecular pictures of portions of the solutions in (a) and (b), showing how they differ. 

C17-0046. Concentrated aqueous HCl has a concentration of 12.1 M. Calculate the concentrations of all ions present in a solution prepared by pipetting 1.00 mL of concentrated HCl into a 100-mL volumetric flask and filling to the mark. 

---