17. w For the following reaction, calculate the [Crt1 in a solution which initially contained 0.0250 M CrCi3 an 0.20 M NaOH. HO6M M 00S.0 lo ztnuoms Cr* (aq) + 4 OH (aq) = Cr(OH)4 = 8.0 x 1029 Jm 00 %3D Im 00.2

17. w For the following reaction, calculate the [Crt1 in a solution which initially contained 0.0250 M CrCi3 an 0.20 M NaOH. HO6M M 00S.0 lo ztnuoms Cr* (aq) + 4 OH (aq) = Cr(OH)4 = 8.0 x 1029 Jm 00 %3D Im 00.2

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.54PAE

See similar textbooks

Related questions

Q: Calculate the solubility of PLCCNy IN a 12M solution of CacCN), KSP FOR Pb (CN) = 4.8x10-51

Q: For nos. 36 - 37, consider a scenario wherein a solution containing 6.25x10 3 M of S2 and 5.63×10 °…

A: The solubility reaction given is, Given: [Cd2+ ] = 5.63 × 10-3 M And [S2- ] = 6.25 × 10-3 M.

Q: The Ksp for Fe(OH)2 at 25°C is 1.6 x 10-14. The solubility of Fe(OH)2(s) in an aqueous solution at…

Q: c) Calculate the solubility (s) of BaSO4 (Ksp = 1.08×10-10) in an aqueous solution with ionic…

Q: A 12-ml. sample of borax solution was titrated with 0.482-M HCL. The endpoint was reached after…

A: Solubility product is mathematical product of it's dissolved ion concentrations raised to the…

Q: A solution contains 0.198 M Pb(NO3)2 and 0.000017M AGNO3. It is intended to separate out the silver…

A: Given that Pb(NO3)2 = 0.198M AgNO3 = 0.000017M

Q: 11. The equilibrium constant for the reaction: AgBr(s) = Ag*(aq) + Br (aq) is the solubility product…

Q: Example: Using activities, find the concentration of OH in a solution of 0.075M NaCIO, saturated…

A: Given in question: Ion size (a) of OH- = 350 pm Ion size(a) of Mn2+ = 600 pm Concentration of…

Q: For AgOH, Ksp = 1.5 x 10-8. What is the molar solubility of AgOH in a solution containing 0.1 M of…

A: Ksp is the solubility product equilibrium constant.

Q: C. 8.12 d. 3.44 e. 5.28 3. Determine the solubility of the ions that is calculated from the Ksp for…

Q: 51 mL of 0.060 M NaF is mixed with 17 mL of 0.15 M Sr(NO3)2. Calculate the concentration of F- in…

Q: Calculate the MW from the average EM. MW (g/mol) = n(eq/mol) x EM (g/eq) where n is the number of…

A: Interpretation- To determine the MW from the average EM for the given two trials that is given as -…

Q: Consider a saturated Mn(OH) 2 solution. Ksp for Mn(OH) 2 =1.97*10^ -13. a) Calculate the molar…

Q: Calculate the molar solubility in M for Mn(OH)2 in 0.1 M KI. Take activity into consideration. Hint:…

A: Formula used :- Ksp = 4s3

Q: Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. Because…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: Percent variance for Kc for Fe3+ + SCN- Fe(SCN)2+ = 110%, the average value for kc = 186 Percent…

Q: (6) 11. Calculate the molar solubility of silver thiocyanate (Ksp= 1.0 x 10-12), AgSCN, in a. pure…

Q: Sodium sulfate is slowly added to a solution containing 0.0500 M Ca"(aq) and 0.0370 M Ag*(aq). What…

A: The dissociation of Ag2SO4 and CaSO4 is as follows,

Q: 25). The solubility of BiI3 (dissociates to Bi3+ ions and I– ions) is 0.00778 g/L. What is Ksp for…

A: Given : Solubility of BiI3 = 0.00778 g/L.

Q: Equilibrium Concentration Fe[SCN]?* Vol of Fe* Vol of SCN- 0.05 M HNO, (mL) (mL) (mL) 10.00 0.00…

A: The molarity of Fe(NO3)3 solution is 0.200 M. The molarity of NaSCN solution is 0.002 M.

Q: Calculate molar conductance (L = 1000k/C ) of the complex [Co(NH3)4CO3]NO3, if the specific…

A: Reaction: [Co(NH3)4CO3]NO3 ⇌[Co(NH3)4CO3]+ + NO3- Molar conductance is calculated as:…

Q: In this experiment, you will prepare standard solutions for a calibration curve for the formation of…

A: Equivalent dilution: Miliequivalent amount of compound will react and through dilution, the…

Q: The activity of Zn2+ in a saturated solution with Zn(OH)2 with 0.00500 M KNO3 (Ksp = 1.20 X10-17, y…

A: Given: Ksp of Zn(OH)2 = 1.20 X 10-17 γ of Zn2+ = 0.748 And γ of OH- = 0.926

Q: 10. The reaction trans-[CoCl2(en)2]+ + H2 --> cis[CoCl(en)2(H2O)|2+ + Cl- is an example of…

A: HSAB principle : Hard acid prefer to bind with hard base while soft acid prefer to bind with soft…

Q: The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14 . When Na2CO3 is added dropwise…

A: Given : Ksp of CoCO3 = 1.0 X 10-10 Ksp of PbCO3 = 7.4 X 10-14 Concentration of Co2+, [Co2+ ] =…

Q: Solid KSCN was added to a(2.20x10^0) M Co2+ solution so that it was also initially (2.20x10^0) M…

Q: The Ksp of AgCl(s) at a specific temperature is 1.8 × 10^-10 M. The concentration of Cl-(aq) in…

Q: You prepare a saturated solution of AgSCN (Ksp = 1.1 xx 1012). You decide to buffer this solution to…

A: The two equilibrium reactions that will be taking place are given as, 1) AgSCN (s) -------> Ag+…

Q: For nos. 36 37, consider a scenario wherein a solution containing 6.25x10-3 M of S2- and 5.63x10-3 M…

Q: 2. Copper(II) hydroxide is only very slightly soluble in water. The reaction by which it goes into…

A: (A) Ksp for Cu(OH)2 is, Ksp explains the equilibrium of a solid in a saturated solution with its…

Q: For the prelab today, all solutions were made using the procedure as outlined in your lab manual.…

A: Solution Concentration Of [Fe(SCN)2+] (M) = Absorbance/(ε × l) Concentration Of Fe3+ (M) =…

Q: The formation constant for [Cu(CN)2]` is 1.0 × 1016, what is the value of the dissociation constant…

Q: Using an experimentally determined value of 2.4×10−10 for the KspKsp calculate how many milligrams…

A: Ksp or solubility product of a sparingly soluble salt is the product of concentration of its ions in…

Q: calculate the solubility of Zn(CN)2 at 25°c in a.) 0.250 M NaCN b.) sol'n buffered at a basic pH…

A: Zn(CN)2 is a sparingly soluble salt, which dissociates in water as:

Q: 4- For the aqueous Fe(CN), complex K,=1.0 × 10 35 at 25 °C. Suppose equal volumes of 0.0068 M…

A: Equal volume of Fe (NO3)2 and KCN = x L Total volume of solution = (x + x) L…

Q: 11) Will a 0.15 M solution of NH3 be sufficient to keep Zn2+ from precipitating from a solution of…

Q: The Ksp for PbI2(s) is 1.4 × 10-8. Calculate the solubility of PbI2(s) in 0.061 M NaI.

Q: The Ksp of Pb(OH)2 at 25 °C is 1.4 x 10-15. What concentration of NaOH will commence…

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: A solution is prepared that has (EDTA1=0 300 M and (CO,2-1= 0 600 M What is the maximum allowable…

A: (i) In a solution of EDTA-4 and CO3-2, Fe+2 is added. This results in the formation of a complex of…

Q: What mass of ZnS (Ksp = 2.5 x 10-22) will dissolve in 325.0 mL of 0.050 M Zn(NO3)2? Ignore the basic…

A: Since Zn(NO3)2 is completely soluble in water as Zn(NO3)2 -----> Zn2+ + 2 NO3- Hence…

Q: A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+…

A: In saturated solution, []Ag+] = [Cl-] = 1.25 * 10^-5 M gCl ........> Ag+ + Cl- Ksp = [Ag+][Cl-]

Q: The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The…

Q: B. Determination of the Solubility-Product Constant Absorbance [Ag*] of Ag, Cro, 0.217 1.0g 0.928 1.…

Q: For Ni(OH)2 (Ksp = 1.6 x 10 16) dissolved in a 0.033 M NizP2 solution, calculate: %3D a. Solubility…

Q: 1. Calculate the molar solubility of Ag2S (pKsp = 48.70) in a solution maintained at pH 9.00 and…

Q: What should be the pH of the environment for 50% of Ag+ ions to complex in the cyanide (CN¯) anion…

A: The complexation equilibrium is given as:

Q: Calculate the solubility of silver chromate in water: Ag2CrO4 ----------- 2Ag + + CrO42- Express the…

A: Ag2CrO4 dissociates as follows: Let the initial solubility be s. [Ag+] = 2s…

Q: ne formation constant for [Cu(CN)2] is 1.0 x 1016, what is the value of the dissociation constant…

A: Applying concept of chemical constants relationship between two chemical reaction.

Q: 17. In which of the following solutions, Mn(OH)2 has the greatest solubility? (by assuming…

Question

What is the [Cr^3+] in the solution?

17. w For the following reaction, calculate the [Crt1 in a solution which initially contained 0.0250 M CrCi3 an
0.20 M NaOH.
HO6M M 00S.0 lo ztnuoms
Cr* (aq) + 4 OH (aq) = Cr(OH)4
= 8.0 x 1029
Jm 00
%3D
Im 00.2

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Introduction:

VIEW

Calculations:

VIEW

Result:

VIEW

Step by step

Solved in 3 steps with 7 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Extraction of Crude Metal from Concentrated Ore

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before developing. What mass of Na2S2O35H2O (sodium thiosulfate pent hydrate or hypo) in 1.0 L of developer is required to dissolve the AgBr as Ag(S2O3)23- (Kf=4.71013)?
. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.
Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.
You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is reported to have a Ksp value of zero in water at 25C. What does this mean?
Calculate the molar solubility of Ag2S (pKsp = 48.70) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.200 M.H2S: Ka1 = 1.0 x 10-7, Ka2 = 1.2 x 10-15[Ag(NH3)2]+ : Kf1 = 2.04 x 103, Kf2 = 8.13 x 103
The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14. When Na2CO3 is added dropwise to a solution containing 0.010 M Co2+ and 0.010 M Pb2+, which ion will precipitate first? What must the [CO32–] be so that the first ion to precipitate comes out of solution, but the second ion does not?
2. Copper(II) hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is: Cu(OH)2(s) (reaversable) Cu+2 (aq) +2OH-(aq) A) It is possible to dissolve siginificant amounts of Cu(OH)2 in solutions i which the concentrations of either Cu+2 or OH- is very small. Explain why this is true using Ksp. B) Explain why Cu(OH)2 might have very appreciable solubility in 1 M HCl. (Consider the effect of Reaction 3 on the Cu(OH)2 solution reactioin) -reaction 3 =H2O (reverse) H+(aq)+OH-(aq), Kc= [H+][OH-]=1*10-14 AT 25 C
A curious CHEM 32.1 student wanted to determine the levels of Fe (FM = 55.85), Al (FM = 26.982) and Pb (FM = 207.2) in a wastewater effluent from a powerplant near their place. To do so, he obtained 100 mL of the water sample for analysis. After appropriate sample preparation, he added10.00 mL of 0.100 M sodium tartrate to prevent the precipitation of Pb. Then, he added NH3 dropwise, which results to precipitation of hydrated Al(OH)3 and Fe(OH)3. After filtration and washing, the student ignited the residue, giving 0.6127 g dry Al2O3 (FM = 101.96) and Fe2O3 (FM=159.69). When heated under a stream of H2, Al2O3 is unchanged, but Fe2O3 was converted to Fe(s) and H2O(g) , giving a residue that weighs 0.4967 g. Meanwhile, he added excess amount of concentrated H2SO4 in the filtrate, which results to precipitation of PbSO4 (FM = 303.26) weighing0.1317 g after drying. Given these information, calculate the ppm Fe, ppm Al, and ppm Pb in the effluent.
(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L
Sodium sulfate is slowly added to a solution containing (aq)0.0500 M Ca^2+(aq) and 0.0310 M Ag+(aq). What will be the concentration of Ca^2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca^2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage: %
Enter your answer in the provided box. Kf for the complex ion Ag(NH3)2+ is 1.5 × 107 at 25 ° C. Using this information, calculate the value of Δ G o f for Ag(NH3)2+(aq).
(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/L