Explain why ICP-MS is more sensitive than ICP-AES.

Calculate the pH of the solution that results from each of the following mixtures.

140.0mL of 0.26M HF with 220.0mL of 0.30M NaF

Producing polymers with high molecular weights is difficult in step polymerizations. Why is it difficult and which techniques exist to overcome this difficulty?

Determine the pH during the titration of 56.9 mL of 0.385 M hydrofluoric acid (Ka = 7.2×10-4) by 0.385 M NaOH at the following points.

(a) Before the addition of any NaOH

(b) After the addition of 14.0 mL of NaOH

(c) At the half-equivalence point (the titration midpoint)

(d) At the equivalence point

(e) After the addition of 85.4 mL of NaOH

When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C water, the final temperature was measured as 40.8 °C. Assume the density for water is 1.000 g/mL regardless of temperature.

a. Determine the magnitude of the heat lost by the hot water.

b. determine the magnitude of the heat gained by the room temperature water.

c. determine the heat gained by the calorimeter

d. determine the calorimeter constant.

As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the potential to kill weeds effectively. A sparingly soluble salt, Herbigon is dissolved in 1 M acetic acid for technical reasons having to do with its production. You have determined that the solubility product Ksp of Herbigon is 9.50×10−6. Although the formula of this new chemical is a trade secret, it can be revealed that the formula for Herbigon is X-acetate (XCH3COO, where "X" represents the top-secret cation of the salt). It is this cation that kills weeds. Since it is critical to have Herbigon dissolved (it won't kill weeds as a suspension), you are working on adjusting the pH so Herbigon will be soluble at the concentration needed to kill weeds. What pH must the solution have to yield a solution in which the concentration of X+ is 6.00×10−3 M ? The pKa of acetic acid is 4.76.

A concentration cell based on the following half reaction at 312 k ag+ + e- --------> ag srp = 0.80 v has initial concentrations of 1.25 m ag+, 0.221 m ag+, and a potential of 0.04865 v at these conditions. after 8.3 hours, the new potential of the cell is found to be 0.01323 v. what is the concentration of ag+ at the cathode at this new potential? Please explain all the steps used to find the answer.

can get the answer for all these questions

1. Calculate the pH in a solution that is 0.98 M in NaC2H3O2 and 0.56 M in HC2H3O2. (Ka = 1.8 x 10–5)

2. Given 15.0 mL of a buffer that is 0.87 M in HOCl and 0.95 M in NaOCl, what is the pH after 2.0 mL of 0.10 M NaOH has been added? (Ka for HOCl = 3.5  10–8)

3. The molar solubility of Mg3(PO4)2 is 6.26 x 10–6 M. Calculate the value of Ksp for Mg3(PO4)2.

4. A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)

5. You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution? (2pts) [MUST GIVE SOME EXPLAINATION OF ANSWER FOR CREDIT]

a) AgX

b) AgY

c) They are equally soluble in acidic solution.

d) Cannot be determined by the information given.

e) None of these (A-D).

6. Which of the following solid salts should be more soluble in 1.0 M HCl than in water? (2pts) (circle all that apply) [MUST GIVE SOME WORK/EXPLAINATION OF ANSWER FOR CREDIT] a) Na2CO3 b) KCl c) AgBr d) KNO3 e) RbF

9.What is the solubility (s) of Mg(OH)2 (Ksp = 8.9 x 10–12) in 1.0 L of a solution buffered (with large capacity) at pH 9.85

7. The Ksp for Co3(AsO4)2 is 6.8 x 10–29. When 0.20 mL of 0.010 M Na3AsO4 is mixed with 0.20 mL of 0.010 M CoCl3, will a precipitate form?

8. What is the maximum concentration of iodide ions that will precipitate AgI but not PbI2 from a solution that is 6.7  10–3 M each in Ag+ and Pb2+? For AgI, Ksp = 1.5 × 10–16 and for PbI2, Ksp = 1.4 × 10–8 .

10. Calculate the concentration of aqueous ammonia necessary to initiate the precipitation of chromium(III) hydroxide from an equilibrium solution 0.050 M solution of CrBr3. Ksp = 3.0 x 10-29 Kb = 1.8 x 10-5

How much heat in kilojoules is evolved in converting 2.00 mol of steam at 140 ∘C∘C to ice at -20.0 ∘C∘C? The heat capacity of steam is 1.84 J/g∘CJ/g∘C and that of ice is 2.09 J/g∘CJ/g∘C.
Remember that if heat is leaving the system, then q is a negative number and if heat is entering the system, then q is a positive number.

1. a) Does a precipitate form when 0.200 L of 0.15 M Ca(NO₃)₂ is mixed with 0.100 L of 0.120 M NaF? At experimental temperature, K_sp of CaF₂ = 3.9 x 10^-11

b) Calcium hydroxide, Ca(OH)₂, is an important component of many mortars, plasters and cements. Calculate the molar solubility of Ca(OH)₂ in water if K_sp is 6.5 x 10^-6.

c) What is the solubility of Ca(OH)₂ in a 0.20 M solution of Ca(NO₃)₂? K_sp of Ca(OH)₂ is 6.5 x 10^-6

1) If the Ka of a monoprotic weak acid is 2.1

How many grams of NaH₂PO₄ and how many grams of Na₂HPO₄ are needed to prepare 2.0 L of 1.50 M “phosphate buffer” with a pH of about 8.00.

You are given:

For salt form of a weak acid NaH₂PO₄ or weak acid H₂PO₄^-, pK_a = 7.21 and K_a = 6.2 x 10^-8

1 mol Na₂HPO₄ = 142 g Na₂HPO₄

1 mol NaH₂PO₄ = 120 g NaH₂PO₄

Select one:

a. Mass of NaH₂PO₄: 35.5 g and Mass of Na₂HPO₄: 276.1 g

b. Mass of NaH₂PO₄: 70.6 g and Mass of Na₂HPO₄: 392.9 g

c. Mass of NaH₂PO₄: 50.2 g and Mass of Na₂HPO₄: 366.5 g

d. Mass of NaH₂PO₄: 37.9 g and Mass of Na₂HPO₄: 312.8 g

e. Mass of NaH₂PO₄: 75.3 g and Mass of Na₂HPO₄: 408.1 g

A mixture solution of Co(II) and Ni(II) shows an absorbance of 0.500 at 500 nm. What percentage of incident light is absorbed by the solution?

Under the given conditions if 20% of the absorbance is ascribed to the contribution of Co(II), what will the absorbance of Ni(II) be?