Find the pH of a solution made by dissolving 0.195 g of phenol (C6H5OH) in enough water to make 125 mL of solution.

When an ant bites you, the reason it stings is because of an injection of formic acid. What is the pH when 50.00 mL of 0.1480 M formic acid (HCOOH) is titrated with 40.2 mL of 0.1841 M of NaOH? pKa of formic acid = 3.745

Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O .

Suppose 60. g of hydrobromic acid is mixed with 48.8 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

A 110.0 −mL sample of a solution that is 2.8×10^−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.11 M in NaCN. A complex ion forms. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Titanium occurs in the magnetic mineral ilmenite (FeTiO3), which is often found mixed up with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s)+3Cl2(g)+3C(s)→3CO(g)+FeCl2(s)+TiCl4(g)TiCl4(g)+2Mg(s)→2MgCl2(l)+Ti(s) Suppose that an ilmenite-sand mixture contains 22.6 % ilmenite by mass and that the first reaction is carried out with a 91.1 % yield. If the second reaction is carried out with an 86.1 % yield, what mass of titanium can be obtained from 1.30 kg of the ilmenite-sand mixture?

a) Copper solutions are typically blue to blue green in color. What color of light would they be expected to absorb in the greatest amount?

b) Based on your answer to the previous question (hopefully you have the correct answer), what wavelength range would you expect to see the maximum absorption of light (in the visible range)?

c) Given the information that the tartrate ion is the conjugate base of a weak acid, how do you expect the solubility of copper (II) tartrate to be affected by pH?

d) It was an intention to have a common ion experiment with the lab, but it did not work when we tested the experiment. What would the solubility of copper (II) tartrate be in a solution that contains 0.19 M sodium tartrate? (Use the literature for copper (II) tartrate K_sp = 4.0 x 10^-4) Please enter answer in standard notation.

e) Your value for K_sp will not be the same as the literature. It may not even be close. It is likely to be larger than the literature value. What is one logical reason your value may be larger?

Calculate the mass of NaCN that must be added to 250.0 mL of water in order to obtain a solution having a pH of 11.25? [Ka of HCN = 4.9 × 10–10] Also, calculate the % ionization of the of the solution.

Theory of enzymes. [Indicate whether the following statements are true or false by writing T or F in the spaces provided.] _____ Enzymes catalyze reactions by increasing the reaction free energy (ΔG). _____ Enzyme are remarkable for their substrate specificity. _____ Enzyme can convert light energy into chemical or mechanical energy. _____ Catalytic residues in enzymes can include amino acid side chains, RNA bases, and other organic cofactors. _____ Michaelis-Menten kinetic theory only applies to enzymes with single substrates. _____ Enzymes bind transition-state analogs more tightly than substrates. _____ At high substrate concentration, reactions are rate-limited by how rapidly enzymes convert substrates into products. _____ KM = KD when kcat >> k-1 _____ kcat / KM is equivalent to a second-order rate constant. _____ Enzymes can use electrostatics to exceed the rate of diffusion (bimolecular collision of substrate with enzyme’s active site). _____ Drugs that bind to an allosteric site on an enzyme cause a decrease in kcat

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 73 ∘C , where [Fe2+]= 3.70 M and [Mg2+]= 0.310 M .

What is the value for the reaction quotient, Q, for the cell?

What is the value for the temperature, T, in kelvins?

What is the value for n?

Calculate the standard cell potential for

Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)

What is the expected pH of a 0.250 M solution of oxalic acid with Ka = 5.37 x 10^-5 ([H+] = 0.002197) and will the pH increase by one unit if the solution is diluted to 0.0250 M?

Two aqueous solutions are at room temperature and are mixed in a coffee calorimeter. The reaction causes the temperature of the resulting solution to fall below room temperature. Whicch statement is true? A) This type of experiment provides data to calculate deltaErxn B)Energy is leaving the system during reaction C)The products have a lower potential energy than the reactants D) The reaction is exothermic E)None of the above is true

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many liters of H2 would be formed at 636 mm Hg and 17 ∘C if 27.0 g of zinc was allowed to react? How many grams of zinc would you start with if you wanted to prepare 6.85 L of H2 at 284 mm Hg and 28.5 ∘C?

Draw the process of the rusting of iron and note the 4-5 chemical ½ reactions. How do we prevent rusting?

Calculate E cell for the new conditons: How does the voltage change and why? (please explain using Le Chateliers principles)

Mg(s) , Mg+2(0.500M) ; Al+3 (2.500M), Al(s)

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An aqueous solution with a pH of 2.22 is diluted from 2.04 L to 3.92 L. What is the pH of the diluted solution?

Thanks in advance!