Fundamentals Of Analytical Chemistry
9th Edition
ISBN: 9781285640686
Author: Skoog
Publisher: Cengage
expand_more
expand_more
format_list_bulleted
Question
error_outline
This textbook solution is under construction.
Students have asked these similar questions
Nickel sulfate, NiSO 4 , reacts with sodium phosphate, Na 3 PO 4 , to give a pale yellow-greenprecipitate of nickel phosphate, Ni 3 (PO 4 ) 2 , and a solution of sodium sulfate, Na 2 SO 4.. How manymilliliters of 0.375 M N i SO 4 will react with 45.7 mL of 0.265 M Na 3 PO 4 ? . Show balanced chemicalreaction of the problem.
A 3.026 grams of Cu (II) salt is dissolved in water and then diluted to 250 mL in a volumetric
flask. Iodine is liberated when one gram of KI solution is added to 50.0 mL of aliquot sample. A
23.33 mL of 0.04668 M Na,S,O, solution is required to titrate the iodine liberated. Calculate the
weight percent of the Cu in the salt.
(A) 11.43%, just before end point
(B) 12.43%, just before end point
(C) 11.43%, after equivalence point
(D) 12.43%, after equivalence point
The thermodynamic solubility product of A9CN is 6.0×10-17.
(a) What is [Ag+] in a 0.033 M KNO3 solution?
4.0
7.75e-9
mol·L-1
(b) What is [Ag+] in a 0.033 M KCN solution?
4.0 1.81e-16
X mol·L-1
Knowledge Booster
Similar questions
- When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?arrow_forwardConsider the solutions presented: (a) Which of the following sketches best represents the ions in a solution of Fe(NO3)3(aq)? (b) Write a balanced chemical equation showing the p10ducts of the dissolution of Fe(NO3)3.arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forward
- What volume (mL) of 0.0.214 M (NH4)2HPO4 is necessary to precipitate the calcium as Ca3(PO4)2 from 838 mg of a sample that contains 9.74% Ca?arrow_forward(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 0.00336 g of Ag2C2O4 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ag2C2O4.Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?solubility = mol/Larrow_forwardThe solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass of KCl(s) must be dissolved in 150.00 mL of 1.15M Pb(NO3)2 to produce a solution that is just saturated in PbCl2?arrow_forward
- What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?arrow_forward(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/Larrow_forward(5) A titration is setup so that NaOH is in a buret and 25.0 mL of HBr soln is in a flask. The NaOH has a known molarity of 0.250 M. At the end point 36.3 mL of NaOH has been added to the HBr soln. What is the molarity of the HBr? (6) A second titration is performed using the same 0.250 M NaOH in a buret. This time 25.0 mL of an H2S04 soln is titrated. At the endpoint 47.8 mL of NaOH has been added to the H2SO4 soln. What is the molarity of the H2S04? 4arrow_forward
- (i) Silver tarnishes in the presence of hydrogen sulfide (produced by rotten eggs) and oxygen because of the reaction below: 4Ag + 2H2S + O2 → 2Ag2S + 2H2O How many grams of Ag2S could be obtained from a mixture of 0.95 g Ag, 0.140 g H2S and 0.08 g O2 ? (ii) At 20°C the solubility limit of silver(I)sulfate (Ag2SO4) is 0.800 g/100 mL. What is the molarity of such a solution? (iii) What volume in mL of concentrated H2SO4 (18.0 M) must be used to prepare 400 mL of 3.0 M H2SO4 solution?arrow_forward11. (ii) A student was given 400 cm of aqueous ammonia solution, NH,(ag), The student was asked to determine how many moles of NH, had been dissolved to prepare the solution. The student titrated 25.0cm of NH.(ag) and found that it reacted exactiy with 32.5cm3 of 0.100 mol dm sulturic acid. The equation for this reaction is shown below. 2NH,(aq) + H,SO,(aq) → (NH)SO,(aq) Calculate the amount, in moles, of NH, in the original 400 cm3 solution. mol answer =arrow_forward(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/Larrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning