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3125g sample of primary standard Na2CO3 was treated with 40ml of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 10.12ml of dilute NaOH. In a separate experiment, it was established that 27.43 ml of HClO4 neutralized the NaOH in a 25ml portion. Calculate the molarities of the HClO4 and NaOH.
What is the pH of a buffer solution containing 0.155 mol dm-3 of benzoic acid and 0.315 mol dm-3 sodium benzoate.
The vapor pressure of a solution containing 5.40 g of a nonvolatilesubstance in 90 g water is 23.32 torr. What is the molar mass of the solute?
Need help figuring out the proper steps on how to solve -What volume of 1.25M HCl in liters is needed to react completely
Pure solid NaH2PO4 is dissolved in distilled water, making 100.0ml of solution. 10 ml of this solution is diluted to 100.00 ml to prepare the orignal phosphare standard solution
A graduated cylinder contains 148 of water. A 17.0 piece of iron (density = 7.86 ) and a 19.0 piece of lead are added. What is the new water level in the cylinder?
Hydrogen peroxide (H2O2) decomposes according to the equation H2O2(l) ? H2O(l) + (1/2)O2(g). Calculate Kp for this reaction at 25oC. (Ho = -98.2 kJ/mol, So = 70.1 J/K•mol)
A piece of metal that has a density of 5.2 g/cm3 and a mass of 100 g was placed in a full jar of water. How many mL of water spilled out of the jar?
A 0.4000M solution of nitric acid is used to titrate 50.00mL of 0.237M barium hydroxide. (Assume that volumes are additive). a) Write a balanced net ionic equation for the reaction that takes place during titration.
When 5.6 grams of NaCl are dissolved in enough water to create a 125-gram solution, what is the solution's concentration, expressed as a percent by mass?
celcius of a solution prepared by dissolving 0.0550 mole of a sodium acetate in 1.00 L of 0.250 M acetic acid.
what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10-13.
what is the total pressure in the reaction flask at the end of the reaction? What are the partial pressures of the gases in the flask? 6A(g) + 2B(g) %u2192 2A3B(g)
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