Complete the following table:
| Mass | Mol | Volume | ||
| Solute | Solute | Solute | Solution | Molarity |
| KNO3 | 23.5g | _____ | 127.0mL | _____ |
| NaHCO3 | _____ | _____ | 260.0mL | 0.150M |
| C12H22O11 | 57.38g | _____ | _____ | 0.120M |
Part A
Complete the row for KNO3.
Enter your answers numerically separated by a comma.
Part B
Complete the row for NaHCO3.
Enter your answers numerically separated by a comma.
Part C
Complete the row for C12H22O11.
Enter your answers numerically separated by a comma.
In: Chemistry
1.What is the solubility of CoCO3(s) in solution that is well-buffered at pH 4.0?
(CoCO3: Ksp=1X1010, H2CO3: Ka1 = 4.45 x 10-7; Ka2= 4.69 X 10-11)
In: Chemistry
Hydrogen chloride can be made in the labatory by the reaction of sodium chloride and sulfric acid!
___NaCl(s)+______H2SO4(aq)____HCl(aq)_____Na2SO4(aq)
Blance the above equation
If 35. g of NaCl are used , How many grams of H2SO4 are required for a complete reaction
If 35. g of NaCl are used , and only 8.6g of HCl are isolated what is the percentage yield of HCl
If only 8.6 g of HCl are obtained , How many grams of Na2SO4, must have been formed.
In: Chemistry
What initial volume (in mL) will 0.00660 mol of hydrogen gas occupy at a pressure of 0.907 atm and a temperature of 9°C? If you heat the sample up to 45°C and maintains a constant pressure, what is the final volume (in mL)?
In: Chemistry
You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.250 M HCl.
(a) How many mL of acid must be added to reach the equivalence point?
(b) What is the pH of the solution before any acid is added?
(c) What is the pH of the solution after 5.00 mL of acid has been added?
(d) What is the pH of the solution at the equivalence point of the titration?
(e) What is the pH of the solution when 30.00 mL of acid has been added?
In: Chemistry
How does sodiums structure determine its properties?
In: Chemistry
A volume of 6.0 mLs of 4.0 N NaOH (FW = 40g/mol) is added to a solution containing 2.50g of tri-protonated Lysine Acid (FW = 147 g/mol). What is the pH of the final solution?
In: Chemistry
A mixture of 0.750 atm ClF3 , 0.554 atm F2 , and 0.394 atm ClF is heated in a closed vessel to 700 K .
ClF3(g)↽−−⇀ClF(g)+F2(g)Kp=0.140 at 700 K
Calculate the equilibrium pressure of each gas at 700 K .
In: Chemistry
Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of a 0.10 M solution of aspirin (acetylsalicic acid, Ka = 3.0 × 10–4) solution.
| A. |
2.9 |
|
| B. |
10.5 |
|
| C. |
4.1 |
|
| D. |
3.5 |
|
| E. |
1.8 |
In: Chemistry
Calculate the amount of heat that must be absorbed by 50.0 grams of ice at -12.0oC to convert it to water at 20.0oC. (specific heat capacity of ice = 2.09 J/g.K; specific heat capacity of liquid water = 4.18 J/g.K; specific heat capacity of water vapor = 1.84 J/g.K; heat of fusion of ice = 334 J/g
In: Chemistry
Some NH4I is palced in a reaction placed in a closed container, which is then heated to 400 deg. C. If the total pressure in the container is (7.47x10^2) , mm Hg, what is the value of Kp. Remember to convert the pressures to atm's.
In: Chemistry
For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true?
A.ΔG is positive for the reaction at 298 K.
B.The change in entropy is the driving force of the reaction.
C.ΔG is temperature independent.
D.The direction of the reaction may be reversed at high temperatures.
E.At high temperature, ΔH becomes positive.
In: Chemistry
What is the mass of potassium oxalate monohydrate and
iron (III) chloride required to synthesize 3g of potassium tris
(oxalato)iron (III). water should not be included in
equation.
Please include equation and explain in detail. thank you!
In: Chemistry
What is chemical equilibrium? Describe the factors that can affect chemical equilibrium, including the presence of catalysts. Explain Le Châtelier’s principle and explain how chemists might use it to increase the amount of products produced in a reaction. (Equilibrium)
In: Chemistry
You have a concentration cell in which the cathode has a silver
electrode with 0.10 M Ag+. The anode also has a silver electrode
with Ag+ (aq), 0.050 M S2O3^2-, and 1.0 x 10^-3 M Ag (S2O3)2^3-.
You read the voltage to be 0.76 V
a. Calculate the concentration of Ag+ at the anode.
b. Determine the value of the equilibrium constant for the
formation of Ag(S2O3)2 ^3-.
Ag+ (aq) + 2S2O3 ^2- (aq) --> Ag(S2O3)2 ^3- (aq) K=?
In: Chemistry