The solubility of barium carbonate, BaCO3, is 0.0100 g/L. Its molar mass is 197.3 g/mol. What is the Ksp of barium carbonate?
In: Chemistry
Calculate the pH of a 0.51 M CH3COONa solution. (Ka for acetic acid = 1.8x10^-5)
In: Chemistry
Assume you are carrying out the titration of 50 mL of a 0.025 M solution of acetic acid with 0.1023 MNaOH. Acetic acid has aKaof 1.8×10−5.
(a) Calculate the pH of the solution at V= 0, V= 0.3Veq, V=Veq, and V= 1.2Veq. (Veq is the equivalence point volume)
(b) If a phenolphthalein indicator was used in this titration, where would the apparent endpoint occur? Assume the apparent endpoint would occur at the end of the color range of the indicator (pH’s of 8.0-9.6).
In: Chemistry
1)
A 1.0-L buffer solution is 0.125 M in HNO2 and 0.180 M in NaNO2.
Part A
Determine the concentrations of HNO2 and NaNO2 after addition of 1.5 g HCl.
Express your answers using three significant figures separated by a comma.
Part B
Determine the concentrations of HNO2 and NaNO2 after addition of 1.5 g NaOH.
Express your answers using three significant figures separated by a comma.
Part C
Determine the concentrations of HNO2 and NaNO2 after addition of 1.5 g HI.
Express your answers using three significant figures separated by a comma.
2)
A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer?
A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer?
| adding 0.050 moles of LiC2H3O2 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| adding 0.050 moles of NaOH | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| adding 0.050 moles of HC2H3O2 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| adding 0.050 moles of HCl | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
|
None of the above will destroy the buffer. 3) Part A Write a balanced equation for the dissolution of CaCO3. Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Write an expression for Ksp for the dissolution of CaCO3. Write an expression for for the dissolution of .
|
In: Chemistry
What is the potential of a galvanic cell made up of Cd/Cd2+ and Ag/Ag+ half-cells at 25
In: Chemistry
Show the cationic poymerization of tetrahydrofuran, using phosphorous pentafluiride/water as catalyst.Prove, based on the mechanism, that phosphorous pentafluride/water is indeed a catalyst and not an initiator.
In: Chemistry
In the reaction MnO4- + 8H+ + 5e- Mn2+ + 4H20, the manganese in 3.95 grams of KMnO4 is reduced to Mn2+. How many coulombs of charge must have been transferred to the permanganate ion
In: Chemistry
Calculate the equilibrium constant for each of the reactions at 25 ∘C .
A.) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
B.) O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq)
C.) Br2(l)+2I−(aq)→2Br−(aq)+I2(s)
In: Chemistry
A rigid tank contains 61.5 g of chlorine gas (Cl2) at a temperature of 77°C and an absolute pressure of 6.00 × 105 Pa. Later, the temperature of the tank has dropped to 34°C and, due to a leak, the pressure has dropped to 3.90 × 105 Pa. How many grams of chlorine gas have leaked out of the tank? (The mass per mole of Cl2 is 70.9 g/mol.)
In: Chemistry
Suppose you made a copper-nickel cell where the copper was the cathode and the nickel was the anode. You add a 0.5000 M solution of copper nitrate on the cathode side and a 3.000 M solution of nickel nitrate on the anode side. What is the voltage of the cell under these conditions? The units are volts and use at least 4 significant digits in the answer. The error interval is 0.02 V.
In: Chemistry
In: Chemistry
ice at 0.0 degree C is used to cool water. What is the minimum mass of ice required to cool 325 g of water from 30.5 degree C to 4.0 degree C? (Heat of fusion= 333 J/g; specific heat capacities: ice= 2.06 J/g.K, liquid water= 4.184 J/g.K)
a. 108g b. 125g c. 325g d. 605g e. 1.75x10^4
Show me the full work.
In: Chemistry
How many grams of dipotassium succinate trihydrate (K2C4H4O4·3H2O, MW = 248.32 g/mol) must be added to 780.0 mL of a 0.0348 M succinic acid solution to produce a pH of 5.921? Succinic acid has pKa values of 4.207 (pKa1) and 5.636 (pKa2).
Succinic acid (H2C4H4O4) is a diprotic acid and the succinate ion (C2H4O42–) is the completely deprotonated form of succinic acid. The addition of the succinate ion to the solution results in a buffer. Since the desired pH of the solution is greater than pKa2 for succinic acid, we know that the solution contains a mixture of the succinate ion and the monoprotonated intermediate species (HC2H4O4–).
In: Chemistry
Use the following data on ethanol-chloroform solutions at 35°C to calculate the activity coefficients of ethanol and chloroform based on the deviations from Raoult’s Law. Explain the meaning of your answers.
| c EtOH, liq | 0 | 0.2 | 0.4 | 0.6 | 0.8 | 1.0 |
| Y EtOH, vap | 0.000 | 0.138 | 0.186 | 0.255 | 0.425 | 1.000 |
| Ptot (kPa) | 39.35 | 40.56 | 38.69 | 34.39 | 25.36 | 13.70 |
Can someone help me with this please!? Thank you!!
In: Chemistry
Using 2-bromobutane as your starting material, write a generic equation for each condition indicating the expected products and show the two possible mechanisms for nucleophilic substitutions.
1-bromobutane (n-butyl bromide)
1-chlorobutane
3-bromopropene (allyl bromide)
2-chlorobutane
2-bromobutane (sec-butyl bromide)
2-chloro-2-methylpropane
2-bromo-2-methylpropane (t-butyl-bromide)
chlorobenzene
In: Chemistry