If 11.2 kilograms of Al2O3(s), 52.4 kilograms of NaOH(l), and 52.4 kilograms of HF(g) react completely, how many kilograms of cryolite will be produced?What is the total mass of the excess reactants left over after the reaction is complete?
In: Chemistry
what are the trends of electronegativity, atomic radii, and ionic radii on the peridot table?
In: Chemistry
An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers.
(a) Find the pH of 0.070 M HClO and 0.070 M NaClO.
(b) Find the pH of 0.070 M HClO and 0.105 M NaClO.
(c) Find the pH of 0.105 M HClO and 0.070 M NaClO
(d) Find the pH of 1.0 L of the solution in part (a) after 0.0050 mol NaOH has been added.
In: Chemistry
Each step in the process below has a 70.0% yield.
CH4+4Cl2-->CCl4+4HCl
CCl4+2HF-->CCl2F2+2HCl
The CCl4 formed in the first step is used as a reactant in the second step. If 7.00 mol of CH4 reacts, what is the total amount of HCl produced? Assume that Cl2 and HF are present in excess.
In: Chemistry
For each strong base solution, determine [H3O+], [OH−], pH, and pOH.
Part A 8.86×10−3 M LiOH
Part B 8.86×10−3 M LiOH
Part C 1.14×10−2 M Ba(OH)2
Part D 1.14×10−2 M Ba(OH)2
Part E 2.1×10−4 M KOH
Part F 2.1×10−4 M KOH
Part G 4.8×10−4 M Ca(OH)2
Part H 4.8×10−4 M Ca(OH)2
In: Chemistry
Cd2+ and Pb2+ ions in a polluted water sample are measured by complexation. In a first titration, 50.00 mL of water at pH 10 is titrated by 40.09 mL of 0.004870 M EDTA. In a second titration, a 75.00 mL aliquot of water is first treated with an excess of KCN to mask the cadmium in Cd(CN)4 2- before being titrated by 31.44 mL of the same EDTA solution. Calculate the concentrations of Cd2+ and Pb2+ in the polluted water sample. Cd2+ + 4 CN- <===> Cd(CN)4 Kf = 1.0 x 10^19 Cd2+ + Y4- <===> CdY2- Kf = 2.9 x 10^16 Pb2+ + Y4- <===> PbY2- Kf = 1.1 x 10^18 aY4- = 0.36
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What mass of HCl gas must be added to 1.00 L of a buffer solution that contains [aceticacid]=2.0M and [acetate]=1.0M in order to produce a solution with pH = 3.73?
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For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH.
Part A
0.20 M NaOH
Express your answer using two significant figures. Enter your answers numerically separated by commas.
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| [OH−], [H3O+]= |
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M |
Part B
Express your answer to two decimal places. Enter your answers numerically separated by commas.
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Part C
1.4×10−3 M Ca(OH)2
Express your answer using two significant figures. Enter your answers numerically separated by commas.
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| [OH−], [H3O+]= |
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M |
Part D
Express your answer to two decimal places. Enter your answers numerically separated by commas.
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| pH,pOH= |
Incorrect; Try Again; 5 attempts remaining
Part E
4.6×10−4 M Sr(OH)2
Express your answer using two significant figures. Enter your answers numerically separated by commas.
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| [OH−], [H3O+]=__________________ | M |
Part F
Express your answer to two decimal places. Enter your answers numerically separated by commas.
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| pH, pOH= |
Part G
8.8×10−5 M KOH
Express your answer using two significant figures. Enter your answers numerically separated by commas.
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| [OH−], [H3O+]= | M |
Part H
Express your answer to two decimal places. Enter your answers numerically separated by commas.
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| pH, pOH= |
In: Chemistry
You are attempting a recrystallization of the world’s only sample of charliebionic acid with a small amount of an unknown impurity. The acid is not soluble at all in water. The acid is very soluble in hot ethanol but only slightly soluble at room temperature. But as the solution cooled to room temperature, no precipitate formed. However, when the solution was cooled in an ice bath solid immediately formed. This solid was dried and the melting point measured. The melting point showed that the impurities remained.
What is the most likely reason that no crystals formed at room temperature?
Why is the charliebionic acid still impure after recrystallization?
Propose a last minute addition to this procedure that might correct this situation and form pure crystals at room temperature from this sample.
In: Chemistry
A 1000.-mL solution of hydrochloric acid has a pH of 1.6. Calculate the mass (g) of HCl dissolved in the solution.
In: Chemistry
1:
A piece of solid magnesium is reacted with hydrochloric acid to form hydrogen gas:
Mg(s) + 2 HCl(aq) à MgCl2(aq) + H2(g)
What volume of hydrogen gas (in mL) is collected over water at 25 °C by reaction of 0.450 g of Mg (AW = 24.3 g/mol) with 5.00 mL of 1.0 M HCl? The barometer records an atmospheric pressure of 762 torr and the vapor pressure of water at this temperature is 23.35 torr.
2:
Given the following balanced chemical reactions and their enthalpies, calculate the enthalpy of reaction for 2C(s) + H2(g) ---> C2H2(g):
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C2H2(g) + (5/2) O2(g) ---> 2 CO2(g) + H2O(ℓ) |
ΔH° = -1299.5 kJ |
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C(s) + O2(g) ---> CO2(g) |
ΔH° = -393.5 kJ |
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H2(g) + (1/2) O2(g) ---> H2O(ℓ) |
ΔH° = -285.8 kJ |
3:
A 10.00 mL aliquot of 0.100 M NaOH is added to 15.00 mL of 0.100 M HCl (don't try this at home, since acids and bases react violently to produce water and heat!) in a coffee cup calorimeter. The initial temperature of the two dilute liquids were both 25.0 ºC and the final temperature of the mixture was found to be 37.8 ºC. What is the (molar) heat of reaction for the neutralization?
4:
The heat of vaporization for toluene is 38.06 kJ/mol and the normal boiling point is 111 ºC. Using the Clausius-Clapeyron equation, calculate the vapor pressure of toluene at room temperature (25 ºC).
5:
What is the equilibrium constant for a weak acid HA that dissociates 1% at an initial concentration of 0.05 M according to the following balanced chemical equation?
HA(aq) ↔ H+(aq) + A-(aq)
In: Chemistry
Compounds A and B have the following vapor pressures:
150oF: PA=600mmHg PB=500mmHg
200oF: PA=1000mmHgPB=950mmHg
Assume that these compounds form ideal solution, calculate the vapor mole fraction of A and the total pressure VLE when the liquid mole fraction of A is 0.50 and the temperature 175oF.
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1000 mol/min of a mixture of 90 mol% air and 10 mol% HCl enters an absorber column and is contacted with a stream of pure water entering the column at the rate 300 moles/min. 90% of HCl in the feed gas is absorbed by water. The two exit streams are gas stream (air+HCl) and liquid stream (water+HCl), respectively.
1. Draw and label a flowchart.
2. Define a basis of calculation.
3. Carry out a degree of freedom analysis and determine flow rates in mole/min and compositions in mole fractions of the exit streams.
In: Chemistry
A) For the reaction: 3A(g)+2B(g)⇌C(g) Kc = 63.4 at a temperature of 377 ∘C .
Calculate the value of Kp. Express your answer numerically.
B) For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 2.91×10−2 at a temperature of 229 ∘C .
Calculate the value of Kc. Express your answer numerically.
C) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.155 at 1774 ∘C .
What is Kp for the reaction at this temperature? Express your answer numerically.
D) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp = 4.40×10−3 at 271 ∘C .
What is K for the reaction at this temperature? Enter your answer numerically.
E) The following reaction was performed in a sealed vessel at 772 ∘C : H2(g)+I2(g)⇌2HI(g)
Initially, only H2 and I2 were present at concentrations of [H2]=3.00M and [I2]=2.80M. The equilibrium concentration of I2 is 0.0400 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
Express your answer numerically.
Thank you so much in advance!
In: Chemistry
Calculate the pH and concentration of all species of malonic acid (C3H4O4) in each of the follwing solutions.
K1=1.42*10^-3, K2=2.01*10^-6
0.100 M NaC3H3O4 solution
0.100 M Na2C3H2O4 solution
In: Chemistry