A solution prepared by mixing 22.4 mL of 0.380 M NaCl and 22.4 mL of 0.380 M KI was titrated with 0.190 M AgNO3 in a cell containing a silver indicator electrode and a saturated calomel reference electrode.

(a) What is [Ag ] when 21.2 mL of 0.190 M AgNO3 have been added? Express your answer as x, where [Ag ] is a quotient having the form Ksp,AgI/x. (b) What is [Ag ] when 67.0 mL of 0.190 M AgNO3 have been added? Express your answer as y, where [Ag ] is a quotient having the form Ksp,AgCl/y. (c) Which of the following expressions shows how cell voltage depends on [Ag ]? (d) The difference between voltages measured when 67.0 mL and 21.2 mL of AgNO3 have been added is 0.3899 V. Using this voltage difference and your answers to questions (a), (b), and (c), calculate the numerical value of the quotient Ksp,AgCl/Ksp,AgI.

Please provide formula!

Molecular weight of chemical A is 40. To make 1 liter of 1molar solution, how much should you use? Specify unit. And to make 50militer of 50millimolar solution, how much should you use?

To make 100 microliter solution that contains 10mililmolar of compund A,B,C, and D, which are in 100milimolar sotck solution individually, how much sterile water and each compound should you mix? Specify unit

A compound came in a tube containing 38.2nanomoles of dry powder. To make 100 micromolar stock solution, how much sterilie water should you add to the tube? Specify the unit.

Describe the 3 types of membranes commonly used to separate the test solution from the internal reference electrode.

Why is the molar heat in a reaction between HCl and NaOH greater than in a reaction between HOAc and NaOH

For a particular reaction at 234.1 °C, ΔG = -832.94 kJ/mol, and ΔS = 923.32 J/(mol·K). Calculate ΔG for this reaction at -105.7 °C.

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.100 M HClO(aq) with 0.100 M KOH(aq). The ionization constant for HClO can be found here.

(a) before addition of any KOH

(b) after addition of 25.0 mL of KOH

(c) after addition of 30.0 mL of KOH

(d) after addition of 50.0 mL of KOH

(e) after addition of 60.0 mL of KOH

Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 7.8×10−4 M . At equilibrium, [FeSCN2+]= 1.7×10−4 M .Calculate the value of the equilibrium constant (Kc).

Hess’s Law Problem: Show your work neatly and methodically.

1. From the enthalpies of reaction PUT *** BY ANY REACTIONS THAT CORRESPOND IN A ΔH FORMATION

H2(g) + F2(g) ---->2 HF(g) ΔH = -537 kJ

C(s) + 2 F2(g)----> CF4(g) ΔH = -680 kJ

2 C(s) + 2 H2(g)------> C2H4(g) ΔH = +52.3 kJ

Calculate ΔH for the reaction of ethylene with F2:

C2H4(g) + 6 F2(g) ----> 2 CF4(g) + 4 HF(g) ΔHRXN = ????

2.Use Hess’s Law to calculate ΔH for the reaction

NO(g) + O(g) ---> NO2(g) given the following information:

NO(g) + O3(g) ---> NO2(g) + O2(g) ΔH = -198.9 kJ

O3(g) ----> 1.5 O2(g) ΔH = -142.3 kJ

O2(g) ---> 2 O(g) ΔH = +495.0 kJ

3.Use Hess’s Law to calculate ΔH for the reaction N2O(g) + NO2(g) ----> 3 NO(g) given the following information:

2 NO(g) + O2(g) ----> 2 NO2(g) ΔH = -113.1 kJ

N2(g) + O2(g) ----> 2 NO(g) ΔH = +180.7 kJ

2 N2O(g) -----> 2 N2(g) + O2(g) ΔH = -163.2 kJ

A 26.0-g aluminum block is warmed to 65.1 ∘C and plunged into an insulated beaker containing 55.5 g of water initially at 22.3 ∘C . The aluminum and the water are allowed to come to thermal equilibrium. (Cs,H2O=4.18J/g⋅∘C , Cs,Al=0.903J/g⋅∘C )

Assuming that no heat is lost, what is the final temperature of the water and aluminum?

T = ??      ∘C     

The pKb values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.44. Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.80 M B(aq) with 0.80 M HCl(aq).

a)before any HCl is added

b)25ml HCl

c)50ml HCl

d)75ml HCl

e)100ml HCl

Use the data below from an electron impact mass spectrum of a pure compound to deduce its structure. Draw your structure in the drawing window.

1.What would be a spectroscopic method to distinguish between the the impurity and the triphenyl methanol?

2.What is one of the common by-products formed in this reaction and how is it separated from the desired product:triphenyl methanol?

3.Provide at least three reasons why the initial reaction to produce the Grignard reagent is likely to fail?

4.Why is it important to buff the magnesium ribbon used for the reaction with bromobenzene?

5.How can you prepare: (a) 3-pentanol, (b) hexanoic acid (c) 3-phenyl 3-propanol.

In a certain chemical reaction, there is a decrease in the potential energy (chemical energy) as the reaction proceeds. (a) How does the total kinetic energy of the particles change? (b) How does the temperature of the reaction mixture change?

Sodium fluoride adopts the NaCl (FCC) structure type. Estimate the lattice energy, ΔU, for NaF using the Born–Lande equation. The bond length for Na–F is 235 pm, and the Madelung constant is 1.7476. The Born exponent of both the cation and the anion is 7.

Consider the titration of a 23.2 −mL sample of 0.115 M RbOH with 0.110 M HCl. Determine each of the following. 1)the initial pH. 2) the volume of added acid required to reach the equivalence point. 3)the pH at 5.9 mL of added acid. 4)the pH at the equivalence point. 5) the pH after adding 4.9 mL of acid beyond the equivalence point. Thank you in advance.