Please help with the following problem. Provide a step by step solution. Solubility and the Common-Ion Effect. In problem 1 it was stated that the molar solubility of PbBr2 in pure water is 1.3 x 10-2 M. Calculate the molar solubility of PbBr2 in A) 0.20 M KBr and in B) 0.20 M Pb(NO3)2 Problem 1 in reference is: The Sol
The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write A) the chemical equilibrium equation that describes the salt partially dissolving in water and B) the solubility product expression. C) Calculate the Ksp value for lead(II) bromide if the molar solubility in pure water is 1.3 x 10-2 M.
LnP = - (delta H vap/ T) (1/T)+C ln P2 = lnP1 + delta H vap / R (1/T - 1/T2) )Gvap=)Hvap - T) Svap G=0. See the attached file.
Calculating Equilibrium Concentrations. Consider the reaction SO2(g) + NO2(g) = NO(g) + SO3(g) at 460 C. What are the equilibrium concentrations of all reactants and products if the initial concentrations are [SO2]o = [NO2]o = 3.00 x 10-3 M and [NO]o = [SO3]o = 4.00 x 10-2 M? The value of the equilibrium constant for the
The Reaction Quotient. The reaction CS2(g) + 4 H2(g) <--> CH4(g) + 2 H2S(g) has an equilibrium constant of 0.28 at 900 C. Fill in the data table below. Please see the attached for the full question.
The Equilibrium Constant. Question: Consider the reaction 2 NO2Cl(g) = 2 NO2(g) + Cl2(g). A 12.0-L container holds these gases at equilibrium. What is the value of Kc for this reaction if there are 1.036 g NO2Cl, 5.962 g NO2, and 4.578 g Cl2 at equilibrium?
The Equilibrium Constant. Question: Consider the reaction SO2Cl2(g) = SO2(g) + Cl2(g), where Kc = 0.078 at 100 Degrees Celsius. What is the molarity of the chlorine gas at equilibrium if the equilibrium mixture contains 2.70 mol SO2Cl2 and 1.30 mol SO2 in a 25.0-L container?
The Equilibrium Constant. Question: Consider the reaction 2 NO(g) + 2 H2(g) = N2(g) + 2 H2O(g). A 3.00-L container is filled with a mixture of 0.300 mol NO, 0.150 mol H2, and 0.300 mol H2O. When the equilibrium is established [NO] = 0.062 M. What is the value of Kc?
At pH 6.00 and pE 2.70, what is the concentration of Fe2+ (mol/L) in equilibrium with Fe(OH)3?
Question: 1 mol of nitrogen and 1 mol of hydrogen are placed in a flask and allowed to come to equilibrium with the product ammonia (NH3). At equilibrium there are .8 moles of nitrogen present. What is the Keq for the reaction?
How do you complete a solubility Ksp problem? What is the solubility of aluminum hydroxide in water at 25 degrees Celsius if the Ksp is 3 x 10^-34? What is the concentration of Hydroxide at equilibrium? What is the concentration of a sulfide ion in a 1L solution of cuprous sulfide to which .03mol of cuprous nitrate has be
Calculating the equilibrium constant. I have had trouble with this problem. The EXACT question asks: Calculate the equilibrium constant at 298K for the following equation. Sn(+2)(aq) + MnO4(-1)(aq) ===> Sn(+4)(aq) + Mn(+2) I understand Kc = (Products^(stoic. coefficients))/(Reactants^(stoic. coeffic
I am having a hard time finding the equilibrium constant for this problem, can anyone help? Determine Equilibrium constant at 298K for: Sn(+2)(aq) + MnO4(-1)(aq) ==> Sn(+4)(aq) + Mn(+2)(aq)
If the formation of products is strongly favoured in this acid base system: HX+(B-)<>HB+(X-) The competing bases are B- and X-, am I correct? B- is a stronger base, am I correct ? Does K for this system have a large or small value and why? How would the equilibrium be affected by the addition of the soluble salt N
The solubility of a product of Ca(OH)2 is 7.9 (10^-6) at 25 C. Will a precipitate form when 100mL of 0.10 mol/L of CaCl2 solution and 50.0 mL of 0.070 mol/L of NaOH solution are combined. Please explain the procedure to this answer by showing all steps.
GIVEN THE EQUILIBRIUM CONSTANT VALUE OF Kc FOR THE FOLLOWING RECTION AT 300 CELSIUS N2(g) + 1/2 O2(g) N2O(g) Kc=3.4 * 10 XY -18(SQUARE ROOT) AT 300 CELSIUS N2O4(g) 2NO2(g) kc=4.6*10(SQUARE RROT OF -3 AT 300 CELSIUS 1/2N2(g) + O2(g)
A mixture of 1 mol of H2O (g) and 1 mol CO (g) is placed in an evacuated 1 liter reaction vessel at 1200 K at equilibrium 0.478 mols of O2 was present. Find Kc CO(g) + H2O (g)<--------> CO2 (g) + H2(g) Is this correct? E = 1-x 1-x <----> 0.478 + x + x 0.478 + x (x) / 1.0-2x+x2 0.478x + x2 It looks li
In the manufacture of sodium carbonate, NaHCO3(s) is decomposed by heating. 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) Kp=0.23 at 100 celsius. 1- If a sample of NaHCO3(S) is brought a temperature of 100
The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 x 10^-3 at 527 deg C. COCl2(g)<--->CO(g)+Cl2(g) Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm Answer should give partial pressures of COCl2, CO, Cl2. I do not understand also what i
Equilibrium process at 686 deg C: C02(g) + H2 <---> CO(g) + H20(g) [CO2] is 0.086 M [H2] is 0.045 M [CO] is 0.050 M [H20] is 0.040 M Calculate Kc for the reaction at 686 deg C. If you add CO2 to increase it concentration to 0.55 mol/L, what will the concentrations off all the gases be when equilibrium is re-establis
1) A 0.223 molar solution of the weak acid, HA, with a pKa of 3.954 is titrated with a 0.142 molar solution of NaOH. What is the pH of the solution at the equivalence point of this titration? 2) 0.1405 mol of potassium cyanide (KCN) is used to prepare 609.1 mL of an aqueous solution. Take the pKa of hydrogen cyanide as 9.38.
A mixture containing 3.9 moles of NO and 0.88 mole of CO2 was allowed to react in a flask at a certain temp according to the equation: NO(g)+CO2(g) f/r NO2(g)=CO(g) At equilibrium, 0.11 mole of CO2 present. Calculate equilibrium constant, Kc.
The equillibrium constant Kc for the reaction shown is 2.18 x 10^6 at 730 deg. C. H2(g)+Br2(g) <--> HBr(g) Starting with 3.30 moles of HBr in a 12.0 L reaction vessel, calculate the concentration of H2, Br2, and HBr at equil.
At 1000 deg. K, a sample of pure NO2 gas decomposes. 2NO2(g)f/r2NO(g) + O2(g) The equilibrium constant Kp is 158. analysis shows that the partial pressure of O2 is 0.14 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture in atm.
H20(l) f/r H+(aq) + OH-(aq) k1 is forward and K_1 is reverse if k1 = 2.4 x 10^-5 s^-1 and K_1=1.3 x 10^11/M *s Calculate the equilibrium constant K Calculate k=[H+][OH-] and [H+] and [OH-]. There should be four answers.
I am a winemaker and in the course of my work I simply do not understand how to do a calculation of this sort. We usually express acidity (in wine) in terms of titratable acidity in grams tartaric acid per liter. Here is the information that I have: If 500 mg/L of lactic acid is added to distilled water and NaOH is added unti
Solve the following problems using the systematic approach to equilibrium problems. 1. Determine the concentration of Ag+, CN-, and HCN in a saturated solution of AgCN where the pH is fixed at 5.90. 2. Determine the concentration of NH4+, NH3, CH3COOH (acetic acid), and CH3COO- (acetate ion) if 0.0050 moles of ammonium acetate
What is the equilibirum pressure of COCL2 when COCL2 dissociates at 395 degree celcius where Kp = .0444 and the total pressure at equilibrium is 3.00 atm. COCl2 (g) arrow both ways CO (g) + Cl2 (g) Please explain how you get this answer, thank-you.
The equilibrium charge-exchange reaction between hydrogen and deuterium is given by: H2 + 2D+ (arrows) D2 + 2H+ Using the standard reduction potentials for each half reaction given below, determine which isoptope of hydrogen (H or D) prefers to be in the +1 state in aquesous solution under standard conditions. 2D+ + 2e- (righ
Can you please help me determine the identity of this molecule. I know from the IR that it contains a carboxyl group, but I am not quite sure what the HNMR is showing. Can you please help me? See the attached file.