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What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 4.5? Enter your answer to two significant figures. (For example, 0.0090 and 0.0097 each have two significant figures, whereas 0.009 has only one significant figure.)
A 1.000 mol sample of propane, a gas used for cooking in many rural areas, was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 25.000°C and its total heat capacity was 96.94 kJ·°C-1. The ..
What mass of P4 is produced when 41.5 g of Ca3(PO4)2, 26.5 g of SiO2 and 7.80 g of C are reacted according to the equation: 2Ca3(PO4)2 + 6SiO2 + 10C ¼ P4 + 6CaSiO3 + 10C
The precipitate was filtered, dried, and weighed. A total of 2.10 g calcium fluoride was collected. What was the percentage of CsF in the original sample?
10 M solution of chloroacetic acid, ClCH2CO2H, has a pH of 1.95. calculate Ka for the acid.
Write a balanced equation for the reaction. What volume of 0.200M MnO4- solution is needed to titrate 22.5mL of a 0.350M solution of ethanol?
The Ksp of mag fluoride is 6.4x10 -9degree calculate the solubility (in g/l) of mag fluoride in water
the concentrations of the four main individual ionic compouns are 0.48 M NaCl, 0.090 M MgCl2, 0.0250 M CaCl2 and 0.0050 M KCl. what is the total mass of salt in one liter of seawater?
A patient weighs 165 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25 mg of drug per mL of solution. How many mL of the drug should the patient receive?
A 25.0 mL sample of .200 M HF is titrated with .200 M NaOH. What is the pH at the equivalence point?
A 20.29 g sample of impure MgCO3 is completely decomposed at 1000oC in previously evacuated 2.0 L reaction vessel. After the reaction was complete the solid residue had a mass of 15.9 g.
Calculate OH- of each aqueous solution using the following H3o+ a. 1.0 X 10-7m in OH- b.1.0 x 10-5 in OH-
write the balanced equation for the combustion of isooctane (C8H18) to produce carbon dioxide and water. Use the smallest possible integers to balance the equation.
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