Explain why atomic absorption spectroscopy and ion chromatographic (IC) technique are used as complementary techniques for water analysis.

Explain the relationship between oxidation-reduction and voltaic cells. Your answer must include equations.

Cacodylic acid (dimethylarsinic acid, HAsO2(CH3)2) is a common buffer used in biology to prepare and fix biological samples. The pKa of cacodylic acid is 6.3.

Part A What is the pH of a buffer solution prepared by mixing 20.0 mL of 0.0700 molL−1NaOH with 20.0 mL of 0.170 molL−1 cacodylic acid? Express your answer using one decimal place. pH =

Part B What is the pH of the buffer solution in part A after 0.0002 moles of H3O+ was added to the mixture? Express your answer using one decimal place. pH =

The solvent for an organic reaction is prepared by mixing 50.0 of acetone () with 61.0 of ethyl acetate (). This mixture is stored at 25.0 . The vapor pressure and the densities for the two pure components at 25.0 are given in the following table. What is the vapor pressure of the stored mixture?

Draw the structure of protonated histidine and indicate (draw and name) all possible non bonding interactions with water. include H bonding, and Hydration Spheres

For the following reaction, 46.0 grams of iron are allowed to react with 18.4 grams of oxygen gas .

iron(s) + oxygen(g) ---> iron(III) oxide(s)

a. What is the maximum mass of iron(III) oxide that can be formed?

b. What is the formula of the limiting reagent?

c. What mass of the excess reagent remains after the reaction is complete?

1500 pound per hour of a waste mixture of 40% benzene, 50% toluene and 10% of water is burned with 25% excessive air. Determine the total heat released and the percent by volume of each component in the flue gas.
thank you.

Polychlorinated biphenyls (PCBs), which were formerly used in the manufacture of electrical transformers, are environmental and health hazards. They break down very slowly in the environment. The decomposition of PCBs can be represented by the equation:

2C12H4Cl6 + 23O2 + 2H2O --> 24CO2 + 12HCL

Answer parts (a) through (e) below: a) How many moles of water are needed to react 10.0 mol O2?

b) How many grams of HCl are produced when 15.2 mol H2O react?

c) How many moles of CO2 are produced when 76.5 g HCl are produced?

d) How many grams of C12H4Cl6 are reacted when 100.25 g CO2 are produced?

e) How many grams of HCl are produced when 2.5 kg C12H4Cl6 react?

A) A student measures the molar solubility of copper(II) hydroxide in a water solution to be 3.49×10^-7 M.  
Based on her data, the solubility product constant for this compound is  .

B) A student measures the molar solubility of nickel(II) cyanide in a water solution to be 1.91×10^-8 M.  
Based on her data, the solubility product constant for this compound is  .

C) A student measures the molar solubility of silver carbonate in a water solution to be 1.24×10^-4 M.  
Based on her data, the solubility product constant for this compound is  .

Suppose there are two known compounds containing the generic elements X and Y. You have a 1.00 g sample of each compound. One sample contains 0.31 g of X and the other contains 0.40 g of X. Identify plausible sets of formulas for these two compounds. X2Y and X3Y X2Y5 and X3Y5 XY and X2Y X3Y and X4Y XY3 and XY4 XY and X3Y X4Y2 and X3Y

For each of the following reactions, 25.0 g of each reactant is present initially.

Determine the limiting reactant.

2Al(s)+3Br2(g)→2AlBr3(s)

Calculate the grams of product in parentheses that would be produced.
(AlBr3)

Determine the limiting reactant.
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)

Calculate the grams of product in parentheses that would be produced.
(NO)

Determine the limiting reactant.
CS2(g)+3O2(g)→CO2(g)+2SO2(g)

Calculate the grams of product in parentheses that would be produced.
(CO2)

1. If 2.000 g of hydrated magnesium chloride are heated to remove the water of hydration, the anhydrous salt that remains has a mass of 0.9366 g. Determine the following:(A)The mass of water that was lost upon heating. (B)The moles of water that were lost upon heating. (C)The moles of magnesium chloride that remained after heating. (D)The mole ratio for the magnesium chloride and the water. (E)The formulas for this hydrate is ___________________________________________(F)The name for this hydrate is ______________________________________________

P4O10 is classified as an acidic oxide because it

A. reacts with acids to produce a salt.

B. is insoluble in water.
C. reacts with water to produce OH– .
D. gives a solution of phosphoric acid, H3PO4, on dissolving in water.
E. can act as a Lewis base by donating electron pairs.

A 9.59 g sample of calcium sulfide was decomposed into its constituent elements, producing 5.33 g of calcium and 4.26 g of sulfur. Which of the statements are consistent with the law of constant composition (definite proportions)? The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%. The ratio of calcium to sulfur will vary based on how the sample was prepared. The mass ratio of Ca to S in every sample of calcium sulfide is 1.25. Every sample of calcium sulfide will have 5.33 g of calcium. Every sample of calcium sulfide will have 55.6% mass of calcium