14-9. A solution containing 50.0 mL of 0.100 M EDTA buffered to pH 10.00 was titrated with 50.0 mL of 0.020 0 M Hg(CIO4)2 in the cell shown in Exercise 14-B: S.C.E. || titration solution | Hg(1) From the cell voltage E = –0.027 V, find the formation constant of Hg(EDTA)²-.
Q: 12-2. State (in words) what ay4- means. Calculate ɑy4- for EDTA at (a) pH 3.50 and (b) pH 10.50.
A:
Q: 13-22. The arsenic in a 1.203-g sample of a pesticla was converted to H2ASO4 by suitable treatment.…
A: The given data contains, weight of pesticide = 1.203 g. volume of AgNO3=40 ml.Concentration of…
Q: 10. Find the pSr of a 50 ml solution of 0.1 M Sr* at pH 10, after addition of 0, 20, 50, and 100 ml…
A: Solution -
Q: The equivalent conductivity of 0.0108 molar aniline hydrochloride is 118,6 ohm-1 cm-1 . When the…
A: Since you have posted multiple questions, we are entitiled to answer only first question in a…
Q: A volume of 75 mL of 0.060 M NaF is mixed with 25 mL of 0.15 M Sr(NO3)2. Calculate the…
A: Solubility is the tendency of solute which dissolves in a saturated solution. Solubility constant…
Q: Calibration of a glass electrode gave a reading of 139.1 mV with a 0.05 m potassium dihydrogen…
A:
Q: A solution prepared by mixing 22.2 mL of 0.400 M NaCl and 22.2 mL of 0.400 M KI was titrated with…
A:
Q: A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300…
A:
Q: The Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the molar solubility of Al(OH)3?
A: Given Ksp of Al(OH)3 is --- 1.90×10-33 What is the molar solubility of Al(OH)3?
Q: Consider the titration of 25.0mL 0.0100M Sn2+by 0.0500M Tl3+in 1M HCl, using Pt and saturated…
A: The expression of Nernst equation is shown below: Where; Ecell= cell potential E0cell = standard…
Q: Determining Chemical Oxygen Demand You are given a 200-mL sample of surface water from Lake Ontario,…
A: Given, Volume of water sample = 200mL Volume of K2Cr2O7 = 0.2M Volume of K2Cr2O7 = 15.0 mL Time of…
Q: A solution prepared by mixing 22.2 mL of 0.400 M NaCl and 22.2 mL of 0.400 M KI was titrated with…
A: Answer is 7.48 x 10-16 M .
Q: 7-15. A cyanide solution with a volume of 12.73 mL was treated with 25.00 mL of Ni²+ solution…
A: A numerical problem based on quantitative analysis, which is to be accomplished.
Q: An EDTA solution prepared from its disodium salt was standardized using 0.250-g primary standard…
A: The question is based on the concept of quantitative estimation. We have to determine hardness of…
Q: 15-10. Suppose that the Ag | AgCl outer electrode in Figure 15-7 is filled with 0.1 M NaCl instead…
A: Given: Ag/AgCl outer electrode is filled with 0.1 M NaCl instead of saturated KCl. Calibration of…
Q: In which of the following solutions will CdS (Ksp = 1.0 x 10-28) be more soluble than in pure water?…
A: Since any solution which will produce ions which are present in CdS will definitely have solubility…
Q: H2S(aq) is analyzed by titration with coulometrically generated I2 in Reactions 17-3a and 17-3b. To…
A: Charge can be calculated as: Q=It Electrolysis of H2S: H2S→S+H+2e-
Q: 2) Find the activity coefficients for both ions of AgCN in a 500 mL solution saturated with AgCN(s)…
A:
Q: 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of…
A:
Q: 12-E. Suppose that 0.010 0 M Mn²+ is titrated with 0.005 00 M EDTA at pH 7.00. (a) What is the…
A: Equilibrium constant (K) is ratio of concentration of products and reactants raise to its…
Q: Solid aluminum hydroxide (Ksp = 1.3 x 10-33) is added to 3.50 mM Al(NO3)3 solution until there are…
A:
Q: Data: t/°C 20 30 40 50 V NAOH / mL 13.1 26.2 16.0 21.8 *Volume of sample solution for titration: 25…
A: Solubility of benzoic acid in water is not possible as benzoic acid is a non-polar molecule. It can…
Q: Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated…
A:
Q: Consider the titration of 50.00 mL of 0.160 M NH3 with 0.200 M HCl. Calculate the pH at the…
A: Given, Volume of NH3=50.00mL Molarity of NH3=0.160M Molarity of HCl=0.200 M…
Q: What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.0o0? Ksp for Mg(OH)2 is…
A: pH= 12.00 pOH = 14- pH =14-12 pOH = 2 [OH-] = 10-pOH = 10-2 =0.01…
Q: Sixty mL of an impure acid solution was diluted to 500mL. A 30.00mL portion of this solution was…
A:
Q: (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and…
A: [EDTA] = 0.0100 M Volume of titration volume of EDTA =…
Q: Chemistry Table 12-1 Electrode Potential versus SHE in Titrations with 0.100 M Ce* Exercise-Ch. 12…
A:
Q: 50 mL of 0.01 M M²+ is titrated with 0.01 M EDTA. Calculate the value of KMy2- so that when 49.95 mL…
A: EDTA forms stable, watersoluble,1:1 complexes with most of the polyvalent metal ions irrespective of…
Q: Quetion 2 The solubality preduct of Cu(OH), i5 4.8 x 10-20. Calculate the value of pCu", or leg[Cu…
A: Common ion effect: The common ion effect refers to the decrease in solubility of an ionic ppt by the…
Q: Forming Ba(I03)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3.…
A: Here first of all we will determine the limiting reagent by calculating number of moles of each…
Q: What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA…
A: A question based on mole concept that is to be accomplished.
Q: * 14-10 The acid-base indicator HIn undergoes the following reaction in dilute aqueous solution: HIn…
A: A) Given, the molar absorptivities for In- and HIn at 485 nm and 625 nm. By using the beer-lambert's…
Q: 13-20. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced…
A: Mass of sample = 4.912 g Concentration of NaOH = 0.00873 M = 8.73 × 10-3 M Volume of NaOH = 25 mL =…
Q: Find the amount of NH4CI that must be added to give 0.5 dm3 solution with pH = 4.25? [Kb (NH3) = 1.8…
A:
Q: Consider the titration of 25.00 mL of 0.0900 M HNO3 with 0.0750 M KOH. HNO3 + KOH KNO3 - Calculate…
A: mmoles of HNO3 taken for titration = C*V = 0.0900 molL * 25.00 mL = 2.25 mmol Required mole ratio in…
Q: 5-30. Generate a curve for the titration of 50.00 mL of a solution in which the analytical…
A:
Q: Consider the reaction: PBSO4 (s) -> solution is 2.0 x 10s M. Find the value of Ksp. Pb2 (aq) + S0,2…
A: Given reaction: PbSO4 (s) → Pb2+ (aq) + SO42- (aq) The concentration of Pb2+ in the saturated…
Q: A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL…
A: Given : Volume of tap water used = 5.00 mL Volume Na2EDTA.2H2O used = 0.635 mL Concentration of…
Q: A 100.0 mL sample of 0.18 M HCIO, (Strong acid) is titrated with 0.27 M LIOH. Determine the pft of…
A: The pH is to be calculated
Q: The un-ionized form of the weak acid HA does not absorb in the visible region. When it ionizes, its…
A: A question based on equilibrium concept, which is to be accomplished.
Q: What is the solubility of Mn(OH)2 at a pH of 11.37? Ksp(Mn(OH)2) = 1.200e-11.
A: The question is based on the concept of solubility product principle and common Ion effect.…
Q: 6-20. A 4.476-g sample of a petroleum product was burned in a tube furnace, and the SO, produced was…
A: Moles of NaOH = Molarity * volume =0.00923 M * 0.025 L…
Q: Find the conditional formation constant for Sr(EDTA)2- at pH 11.00, where log Kf is 8.72 and ayt- is…
A:
Q: A solid sample containing chloride and with a mass equal to 6.000 g was dissolved in water and…
A: Balanced chemical equation for the given reaction is: Cl- + AgNO3 → AgCl + NO3- This means that 1…
Q: 15- Which is not an error associated with an incorrectly defined pH measurement? a) contact…
A: An error that is not associated with an incorrectly defined pH measurement has to be given,
Q: In which of the following solutions will CdS (Ksp = 1.0 x 10-28) be more soluble than in pure water?…
A: Since any solution which will produce ions which are present in CdS will definitely have solubility…
Q: Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by…
A: From the balanced redox reaction in the acidic medium, concentration of hydrogen peroxide in the…
Q: Report the %w/w KCl and NaBr in the sample.
A: %w/w is used to calculate the concentration. formula, %w/w=mass of element in gramsmass of sample…
Q: Compute the titration curve for Demonstration 16-1, in which 400.0 mL of 3.75 mM Fe21 are titrated…
A:
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
- Compute the titration curve for Demonstration 16-1, in which 400.0 mL of 3.75 mM Fe21 are titrated with 20.0 mM MnO24 at a fixed pH of 0.00 in 1 M H2SO4. Calculate the cell voltage at titrant volumes of 1.0, 7.5, 14.0, 15.0, 16.0, and 30.0 mL and sketch the titration curve.A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.For the titration of 100mL of 0.001M NaCl (Cl-) with 0.0100M AgNO3 (Ag+), calculate the voltage at VAg+ = 0.5, 10.0, and 15.0mL Ksp (AgCl) = 1.8 x 10-10.
- A 100.0 mL100.0 mL solution of 0.0200 M Fe3+0.0200 M Fe3+ in 1 M HClO41 M HClO4 is titrated with 0.100 M Cu+0.100 M Cu+, resulting in the formation of Fe2+Fe2+ and Cu2+Cu2+. A PtPt indicator electrode and a saturated Ag∣∣AgClAg|AgCl electrode are used to monitor the titration. Write the balanced titration reaction. titration reaction: Fe3++Cu+⟶Fe2++Cu2+Fe3++Cu+⟶Fe2++Cu2+ Complete the two half‑reactions that occur at the PtPt indicator electrode. Write the half‑reactions as reductions. half‑reaction: ?∘=0.161 V half‑reaction: ?∘=0.767 V Select the two equations that can be used to determine the cell voltage at different points in the titration. ?E of the Ag∣∣AgClAg|AgClelectrode is 0.197 V.0.197 V. ?=0.767 V−0.05916×log([Cu2+][Cu+])−0.197 V E=0.767 V−0.05916×log([Cu2+][Cu+])−0.197 V ?=0.767 V−0.05916×log([Fe3+][Fe2+])−0.197 V E=0.767 V−0.05916×log([Fe3+][Fe2+])−0.197 V ?=0.767 V−0.05916×log([Cu+][Cu2+])−0.197 V E=0.767…A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationA piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.
- Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated calomel electrodes , calculate E at following volumes of Tl3+ : 1, 5 and 10mlA 50 mL sample solution containing 8-hydroxyquinoline (MW: 145) was analyzed by adding 25 ml, 0.1 M KBrO3, excess KBr and acidified. The mixture was left for 10 minutes in dark place. After this time KI in excess was added followed by titration with 27.9 mL, 0.05 M thiosulfate standard solution. Write balance equations? What is the percent w/v 8-hydroxyquinoline in sample?1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.
- H2S(aq) is analyzed by titration with coulometrically generated I2 in Reactions 17-3a and 17-3b. To 50.00 mL of unknown H2S sample were added 4 g of KI. Electrolysis required 812 s at 52.6 mA. Find the concentration of H2S (mg/mL)in the sample.A 50.0 mL of 3.1% (w/v, g/mL) NaOH solution is mixed with 40.00 mL of 1.2% (w/v, g/mL) Na2CO3 solution. What volume of 0.087 M HCl will be required to titrate the resultant solution to bromocresol green indicator end point (Bcg pH transition range 3.8-5.4, Fwt of NaOH=40 g/mol, Na2CO3= 105.99 g/mol).Excess Ca(OH)2 is shaken with water to produce a saturatedsolution. The solution is filtered, and a 50.00-mL sampletitrated with HCl requires 11.23 mL of 0.0983 M HCl toreach the end point. Calculate Ksp for Ca(OH)2.