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Calculate the pH of a buffer solution made by adding .83 g of sodium acetate trihydrate [(NaC2H3O2)-3 H20] to 50 ml of .100 M acetic acid. Assume there is no change in volume on adding the salt to the acid. pKa for acetic acid is 4.7
How many Grams of NH3 are consumed when 12.5 grams of 02 react completely in the following equation? I am not sure exactly how to solve this.
Which of the compounds contain chiral centers? (you may choose more than one answer)
What is the equilibrium constant for the reaction N2(g) + 3 H2(g) ?? 2 NH3(g) at this temperature?
How many moles of OH were used to reach the end point? How many moles of H from HCl were used for back titration? How many moles of H from the solid were neutralized? What is the equivalent mass of the unknown acid?
calculate the concentration of sodium formate that must be present in a 0.10 M solution of formic acid to produce a buffer with a pH of 3.80
Table salt (NaCl) and sugar (C12H22O11) are accidentally mixed A 5.00g sample is burned and 2.20-g of CO2 are produced. What is the mass percentage of the table salt in the mixture.
Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.
how efficient is the extraction of tea leaves containing 1.0g of caffeine with two 30mL portions of chloroform over that of a single-step extraction? KD= 8.36 at 25 C)
At high temperatures, ammonia can react with oxygen according to the following unbalanced reaction: NH3 + O2 ---> NO + H2O If 5.76 moles of NH3 react with 12.2 moles of oxygen
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.110 M HClO(aq) with 0.110 M KOH(aq).
The partial pressure of O2 in air at sea level is 0.21 atm. Using Henry's law, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20C and an atmosphere pressure of 650 torr.
If 30mL of 6.8M H2SO4 was spilled , what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid.
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