A solution is made by mixing 12.5 g of Sr(OH)2and 40.0 mL of 0.200 M HNO3.

a. Calculate the concentration of OH− ion remaining in solution.

b.Calculate the concentration of Sr2+ ion remaining in solution.

c.Calculate the concentration of NO−3 ion remaining in solution.

d. Is the resultant solution acidic or basic?

What is the difference between biochemical, pharmaceutical, and diagnostic chemical reactions in healthcare?

What is a specific example that exists for each of these chemical reaction types above and why might it be of importance to healthcare professionals?

List a balanced chemical equation for each of these chemical reaction types and explain how it is used in your example above.

i need references to APA format

Estimate the fugacity for each species in the following gases at 290 K and 800 bar:

(a) Pure oxygen;

(b) Pure nitrogen;

(c) Oxygen and nitrogen in a 30% mol O2 and 70% mol N2 mixture using the Lewis-Randall rule

(d) Oxygen and nitrogen mixture in part (c) using van der Waals equation of state.

From a molecular viewpoint, where does the energy absorbed in an endothermic chemical reaction go?

Complete the table using the following data:

IO₃^- (aq) + 6S₂O₃^2- (aq) + 6H₃O⁺ (aq) --> I^- (aq) + 3S₄O₆^2- (aq) + 9H₂O (l)

Express the concentration of a 0.0400M aqueous solution of fluride,F-, in mass percentage and in parts per million.Assume the density of the solution is 1.00f/mL.

When Vo = 0.5× Vmax, [S] = 1× Km. Which of the following is true when [S] = 4× Km?

V0 = 40% of Vmax

none of these

V0 = 8% of Vmax

Vo = 80% of Vmax

Vo = 4% of Vmax

Question 1: Using Hard/Soft Acid/Base Concepts (HSAB) please decribe the following

a) Dimethylmercury, Hg(CH3)2, is one of the strongest known neurotoxins. Is it safe to mix mercuric fluoride, HgF2, with methyl lithium, LiCH3? Explain your decision.

b) Dimethylmagnesium, Mg(CH3)2, reacts violently with water, while Hg(CH3)2 is remarkably stable in aqueous environment. Explain this observation and provide a chemical equation for the reaction involving Mg(CH3)2.

Why is the “standard additions” a better method compared to the external calibration method?

Nitrous acid has a Ka of 4.0 * 10-4. in 1.00 L of solution, 0.670 moles of nitrous acid (HNO2) are added to 0.281 moles of NaOH. What is the final pH?

1. A 0.4243-g sample of CaCO 3 is dissolved in 12 M HCI and the resulting solution is diluted to 250.0 mL in a volumetric flask.
a) how many moles of the CaCO 3 are used (formula mass = 100.1)?
b) what is the molarity of the CA 2+ in the 250 mL of solution?
c) How many moles of Ca 2+ are in a 25.00 mL aliquot of solution in lb?

2. 25.00 mL aliquots of the solution from problem 1 are titrate with EDTA to the Eriochrome Black T end point. A blank containing a small measured amount of Mg 2+ requires 3.21 mL of the EDTA to reach the end point. An aliquot to which the same amount of the Mg 2+ is added requires 24.95 mL of the EDTA to reach the end point.
a) How many milliliters of EDTA are needed to titrate the CA 2+ ion in the aliquot?
b) How many moles of the EDTA are there in the volume obtained in part A?
c) What is the molarity of the EDTA solution?

3. A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg 2+ is added as previously, and the volume of EDTA required is 31.84 mL.
a) What volume of EDTA is used in titrating the Ca 2+ in the hard water?
b) How many moles of EDTA are there in that volume?
c) How many moles of Ca 2+ are there in the 100 mL of water?
d) If the Ca 2+ comes from CaCO 3+ How many moles of CaCO 3 are there in one liter of the water? How many grams of CaCO 3 are present per liter of the water?
e) If 1 ppm CaCO 3 = 1 mg per liter, what is the water hardness in ppm CaCO 3?

A 25.0 mL sample of 0.125 molL−1 pyridine (Kb=1.7×10−9) is titrated with 0.100 molL−1HCl.

Calculate the pH at one-half equivalence point.

Calculate the pH at 40 mL of added acid.

Calculate the pH at 50 mL of added acid.

A CHEM 2242 student dissolved 69.322 g of an unknown monoprotic acid in a 250 mL volumetric flask. The student then transferred 5.00 mL of this solution into a conical flask and diluted the 5.00 mL with another 85.00 mL of DI H₂O. Using the second derivative method the student estimated that equivalence occured when 36.86 mL of 0.1066 M NaOH titrant had been added. What is the molarity of the unknown acid solution?

A 80.0 mL sample of 0.0300 M HClO4 is titrated with 0.0600 M CsOH solution. Calculate the pH after the following volumes of base have been added.

(a) 17.2 mL pH = (b) 39.2 mL pH = (c) 40.0 mL pH =

(d) 40.8 mL pH = (e) 74.4 mL pH =

A sample of 7.60L of NH3 (ammonia) gas at 22 ?C and 735 torr is bubbled into a 0.300L solution of 0.400 M HCl (hydrochloric acid).

The Kb value for NH3 is 1.8