The buffer solution produced at the beginning of the Group III procedure is approximately 1.2 M NH.Cl and 1.0M NH,. Calculate the hydroxide ion concentration in this solution. K, for NH, is 1.8 x 10.
Q: In aqueous solution the Cd2+ ion forms a complex with four ammonia molecules. Write the formation…
A: Introduction: The chemical equation shows the reaction between the two or chemical species and their…
Q: Calculate the molar solubility of gallium hydroxide, Ga(OH); (K.p 7.28 x 10 36), in a solution that…
A: Given: The Ksp of Ga(OH)3 = 7.28 * 10-36. The pH of the solution = 3.59.
Q: A buffer is created by adding 0.321 moles of bromoacetic acid (pKa = 2.902) and 0.555 moles of…
A: Given that : Moles of acid (bromoacetic acid) = 0.321 moles Moles of salt (sodium bromoacetate) =…
Q: Strong base is dissolved in 535 ml of 0.400 M weak acid (K = 3.41 x 10-5) to make a buffer with a pH…
A: Given, Ka = 3.41 X 10-5 [HA]initial = 0.4 , Volume = 535 ml pH of buffer solution = 3.94
Q: Write the ion-product expression for barium phosphate. Ksp
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Q: A 1.000 L buffer solution contains 0.250 mol/L NH, and 0.250 mol/L NH,Cl. K = 1.8 x 10* Determine…
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Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…
A:
Q: The solubility product of CaSO4∙2H2O is 2.4 × 10–5. What mass of this salt will dissolve in 1.0 L of…
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Q: 8. A 1.000 L buffer solution contains 0.250 mol/L. NH, and 0.250 mol/L. NH, CL K=1.8x10 Determine…
A: We have to calculate the pH
Q: The molar solubility of chromium(III) phosphate in a 0.106 M chromium(III) acetate solution is M.
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Q: A student decided not to filter the saturated calcium hydroxide solution prior to titration with…
A: Calcium Hydroxide is strong base while hydrochloric acid is also strong acid , when calcium…
Q: The maximum amount of iron(III) sulfide that will dissolve in a 0.238 M sodium sulfide solution is…
A: The concentration of sulfide ion would be 0.238 M by the application of common ion effect. The…
Q: Determine the molar solubility of AgBr in a solution containing 0.110 mol L-1 NaBr. Ksp (AgBr) = 7.7…
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Q: What is the definition of titer? Specifically in analytical chemistry.
A: Explained as follows
Q: A buffer solution is prepared by taking 0.25 moles of acetic acid (pKa = 4.76) and 0.400 moles of…
A: Given: Moles of acetic acid = 0.25 mol Moles of barium acetate = 0.400 mol Volume of solution =…
Q: A buffer solution is prepared by taking 0.400 moles of acetic acid (pKa = 4.76) and 0.250 moles of…
A: The Henderson Hasselbalch equation for acidic buffer solution is given as :
Q: Calculate K from the reaction where silver bromide is dissolved by 6M aqueous ammonia.
A:
Q: Write the solubility product expression for Ag3PO4
A: The solubility reaction of Ag3PO4 is Ag3PO4 (s) -------> 3 Ag+ (aq) + PO43- (aq)
Q: a) Sodium acetate, CH3COONa was hydrolysed in water, H2O. Show the reaction equations involved. What…
A: The given statement is, Sodium acetate was hydrolyzed in water. For that, the corresponding reaction…
Q: Calculate the ratio of pyridine (C3H,N) to it's conjugate acid, the Pyridinium ion (C3H,NH"), CHN in…
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Q: Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP…
A: Answer: According equilibrium mentioned phenolphthalein is a weak acid. As an indicator when it is…
Q: The solubility of AgBr will be greatest in Question 3 options: 0.1 M NaCl 0.1 M NaBr 0.1 M AGNO3…
A: Common ion effect: According to this effect the solubility of an ionic precipitate will decreases if…
Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…
A: Buffer solution - A solution whose pH is not altered to any great extent by the addition of small…
Q: A buffer solution is 0.100 M in both HC7H5O2 and LIC7H5O2 and has a pH of 4.19. Which of the…
A: The buffer solution is that can resist the small change in PH by the addition of acid or base.
Q: Consider a solution of 0.00500 M HBr for numbers 22-24. Determine the following: M 22. equilibrium…
A: [HBr] = 0.005 M
Q: Consider a buffer solution that contains 3.87 M KClO2 which has a Ka value of 0.011 and 5.69 M…
A: Answer: Buffer solution is the type of solution that resists the change in its pH on adding small…
Q: 8. What change in pH would be observed upon the addition of 0.02 mol of HCl solution to (a) the…
A: From henderson hasselbalch equation , pH = pKa + log…
Q: The Ka expression for the H,PO,/HPO;- buffer is given by the equation Ionic strength (µ, M) 0.005…
A: The Ka for the H2PO4-/HPO42- buffer is given by the equation: What is the pH of a 3:4 mixture of ...
Q: A buffer solution that is 0.470 M in HClO and 0.470 M in KCIO has a pH of 7.46. The addition of 0.01…
A:
Q: - The concentration of ammonia (17.031 g/mol) can be determined through back titration. After…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Consider the titration of 60.00 mL 0.120 M NaHCO3 with 0.250 M KOH. a. Determine the pH after…
A: Given, The titration of 60.00 mL 0.120 M NaHCO3 with 0.250 M KOH.When added15.00mL KOH the pH of…
Q: Consider the insoluble compound zinc sulfide , ZnS . The zinc ion also forms a complex with…
A: Solubility means the maximum amount of solute that can be dissolved in a given solvent. Ksp is known…
Q: Calculate the molar solubility of Ca(OH) in a solution buffered at pH = 10, if the solubility…
A: We have to find the molar solubility
Q: solubility-product constant for this salt at 25 °C.
A: Since Ksp of LaF3 = 2X10-19 And the reaction is LaF3 ----> La3+ + 3F- Hence Ksp = [La3+][F-]3
Q: At pH 10.0, only 0.019 g of MgCl2 will dissolve per 1 L of solution. What is the Ksp of magnesium…
A: The pH is given as 10.0 Therefore pOH = 14-pH = 14-10.0 =4.0 Then the pOH = -log[OH-] So, [OH-] =…
Q: Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of solidNaOH to the original…
A: given: volume of solution = 1L no of mole of NaOH= 0.010 mole As the no of mole of NaOH is very…
Q: A 1.48 L buffer solution consists of 0.128 M butanoic acid and 0.338 M sodium butanoate. Calculate…
A:
Q: n aqueous solution the Cd2+ ion forms a complex with four cyanide anions. Write the formation…
A: Transition and inner transition metals form coordinate complexes with neutral or ionic ligands.…
Q: The maximum amount of chromium(III) phosphate that will dissolve in a 0.145 M potassium phosphate…
A:
Q: In a Mohr titration, silver chromate will be produced until essentially all of the halide has been…
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Q: The maximum amount of cobalt(II) sulfide that will dissolve in a 0.110 M cobalt(II) acetate solution…
A: The question is based on the concept of common Ion effect. it states that solubility of weak…
Q: What volume of 0.500 M HNO2 should be added to 500 mL of 0.750 M KNO2, so that the pH of the…
A:
Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pKa = 4.76) and 0.400 moles of…
A:
Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pKa = 4.76) and 0.400 moles of…
A: From the Henderson-Hasselbalch equation:
Q: A solid sample of Zn1OH22 is added to 0.350 L of 0.500 Maqueous HBr. The solution that remains is…
A: The reactions taking place are, HBr first reacts with Zn(OH)2 to give zinc bromide. The excess HBr…
Q: A 5.36g sample of NH4CI was added to 25ml of 1.00 M NaOH and the resulting solution was diluted to…
A: Given that: Mass of NH4CI = 5.36 g Molarity of NaOH = 1.00 M Volume = 0.100 L To find: pH of…
Q: Strong base is dissolved in 695 ml. of 0.600 M weak acid (K, 3.67 x 10) to make a buffer with a pH…
A: Given: Ka of acid = 3.67 × 10-5 Concentration of HA = 0.600 M Volume of solution = 695 mL = 0.695 L…
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- If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/LCan cadmium (II), and mercury (II) be separated quantitatively by precipitation as sulfides from a solution that is 0.15 M cadmium nitrate and 0.10 M in mercuric ions? If possible, what range of sulfide concentration is permissible? Do you expect any interference from the formation of hydroxides of both heavy metals? CdS (144.46); Ksp = 1.0 x 10 ^ -27HgS (232.66); Ksp = 2.0 x 10 ^ -53 HINT: Determine the concentration at which each of the cations start to precipitate out of solution. >Quantitative precipitation means 1/1000 remains in solution.Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of these
- In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.Find the solubility of Cr(OH)3 in a buffer of pH 13. (Ksp of Cr(OH)3 is 6.3x10-31; Kf of Cr(OH)4- is 8.0x1029) Write the chemical equation & the ion-product expression for the dissolution of Cr(OH)3 Write the chemical equation & the equilibrium expression for the formation of Cr(OH)4- Write the overall chemical reaction & calculate its associated equilibrium constant Koverall Calculate the solubility of Cr(OH)3 in a high capacity buffer with a pH 13
- Sometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.1. What are some precautions that should be observed when collecting samples for DO determination, to ensure the amount of oxygen in the sample is representative of the DO at the site? 2. The standard Winkler method uses sodium iodide and sodium azide to be added at the same time as sodium hydroxide. What is the purpose of sodium azide? 3. Chlorinated tap water contains both chlorine (Cl2) and hypochlorite (OCl-) does the presence of these species affect DO results? Write equations to represent their individual interactions. 4. What effect would nitrate (NO2-), a common constituent of polluted water, have on DO results? Write a balanced equation for its interaction. 5. What is meant by seawater intrusion in drinking water supplies? How does this happen? What are some consequences of these phenomena?A 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.
- In complexation volumetry, classify the statements below as true or false.Justify the one(s) that you judge to be “false”.a) When preparing an EDTA solution, to be used as a titrant of Ca2+ ions, it is necessary to add a small amount of Mg2+ in the solution.b) A metallochromic (Ind) indicator is a substance that forms colored complexes with metallic ions. The colors of these complexes are always the same as the colors of the free forms of these indicators.c) In order for the titration of a metal (Me) with EDTA to be carried out, it is necessary that the Me-EDTA complex has a stability constant greater than that of the Me-Ind complex.d) In determining the partial hardness of a hard water sample with EDTA solution, murexide is used as an indicator at pH 10.Use solubility to calculate Ksp- The solubility of Co(OH), is measured and found to be 3.76*10^-4 g/L. Use this information to calculate a Ksp Value for cobalt(Il) hydroxide. Ksp = Calculate solubility in the presence of a common ion. Calculate the solubility of ZnCO3, (a) in pure water and (b) in a solution in which [CO3^2-] = 0.202 M. Solubility in pure water = M Solubility in 0.202 M CO3^2- =MA 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500 mL. A 25.00 mL aliquot was titrated with 0.0025 M KMnO4 spending a volume of 9.32 mL. Subsequently, a 25.00 mL aliquot was passed through a Walden reducer to later titrate it with the same permanganate solution, using a volume of 14.15 mL for the titration. Determine the percentage of Fe(III) in the sample and report it as % Fe2O3
