When 22.0 mL of a 3.68×10-4 M silver nitrate solution is combined with 25.0 mL of a 1.80×10-5 M sodium sulfate solution does a precipitate form? (yes or no)

For these conditions the Reaction Quotient, Q, is equal to ____?

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH.

A.)Calculate the pH at 0 mL of added base.

B.)Calculate the pH at 5 mL of added base.

C.)Calculate the pH at 10 mL of added base.

D.)Calculate the pH at the equivalence point.

E.)Calculate the pH at one-half of the equivalence point.

F.)Calculate the pH at 20 mL of added base.

G.)Calculate the pH at 25 mL of added base.

Consider the following reaction between sulfur trioxide and water:

SO3(g)+H2O(l)=H2SO4(aq)

A chemist allows 61.5 g fo SO3 and 11.2 g of H2O to react. When the reaction is finished, the chemist collects 51.0g of H2SO4.

1) Determine the theoretical yield for the reaction.

2) Determine the percent yield for the reaction.

Which of the following descriptions and/or equations best represents the enthalpy change of a system? There may be more than one correct answer. A. The heat absorbed or released during a phase change or chemical reaction at constant pressure B. The work done on or by a phase change or chemical reaction at constant pressure C. deltaH = deltaE + PdeltaV D. deltaE = q + w E. H= E + PV F. The heat sborbed or released during a phase change or chemical reaction at constant volume G. The amount of energy required to raise the temperature of 1 mole of a substance by 1 degree C at constant pressure H. The sum of the internal energy and the pressure-volume product of a system

why are Co2+ complexes labile with respect to ligand exchange while Co3+ complexes are relatively inert?

1) Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction

NH4HS(s)⇌NH3(g)+H2S(g)

This reaction has a K value of 0.120 at 25 ∘C.

an empty 5.00-L flask is charged with 0.400 g of pure H2S(g), at 25 ∘C.

What is the initial pressure of H2S(g) in the flask?

The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal.

A 0.160-mole quantity of M(NO3) is added to a liter of 0.720 M NaCN solution. What is the concentration of M ions at equilibrium?

Glycogen is the body’s storage form of glucose. When glycogen is degraded, glucose 1-P is formed. Glucose 1-P can then be isomerized to glucose 6-P. Starting with glucose 1-P and ending with two molecules of pyruvate, what is the net yield of glycolysis in terms of ATP and NADH formed?

The formation of a dipeptide is the first step toward the synthesis of a

protein molecule. Consider the following reaction:

glycine (aq) + glycine (aq) à glycylglycine (aq) + H2O (l)

Given that the standard formation free energies for glycylglycine (aq), glycine (aq) and

water are respectively – 487.9 kJ/mol, – 315.9 kJ/mol and – 237.13 kJ/mol, calculate

DRGo’ and the equilibrium constant at 298 K, keeping in mind that the reaction is carried

out in an aqueous buffer solution. Assume that the value is essentially the same at 310K.

What conclusion can you draw from your result?

Give two reasons why the Co3+ substitution mechanism is dissociative/ID instead of associative/IA

A student collected the following data while using the procedure described in this module: 27.13 mL of 1.00 x 10^-2M EDTA soltuion was required to reach the ErioT end point for titration of 25.00 mL of the sample water. After boiling and filtering 100.00 mL of the water, the student diluted the filtrate to 100.0 mL with distilled water. To titrate 25.00 mL of the diluted filtrate, 26.40 mL of 2.00 x 10^-1 M EDTA solution was required. The studetn precipitated the Ca^2 ion as CaC2O4 from 75.00 mL of the water sample and removed the precipitate by filtration. The student then adjusted the water sample volume to 100.0 mL. To titrate 25.00 mL of the diluted filtrate, 7.43 of 1.00 x 10^-2 M EDTA solution was required Calculate the permanent water hardness in terms of total mmol of Ca^2 and Mg^2 ions.

Sketch a titration curve for 50 mL of 0.10 M HCl titrated with 0.15 M NaOH.

Include on the graph:

a) The initial pH

b) The volume of the equivalence point

c) The pH at the equivalence point

d) The pH after addition of 50 mL of NaOH

SHOW STEPS

386 km/s = _______ cm/s ?

386 km/s = ________ m/ms ?

1270 g/L = _______ g/mL ?

1270 g/L = ________ kg/mL ?

615 mK/s = _______ K/s ?

615 mK/s = ________ μK/ms?

2.999 mg/mL = _______ g/L ?

2.999 mg/mL = ________ μg/mL?

1) The reversible chemical reaction

A(aq)+B(aq)⇌C(aq)+D(aq)

has the following equilibrium constant:

K=[C][D][A][B]=5.2

a) Initially, only A and B are present, each at 2.00 mol L−1. What is the final concentration of A once equilibrium is reached?

b) What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol L−1 ?