QI: A: Calculate the solubility product constant for PECI., if 80.0 ml of a saturated solution of PBCI was found to contain 0.3408 g of PhCl; dissolved in it? Discuss your results. (Solubility in 0.3408g/50 ml.) PbCla - Pb +2C1 iu B: What is the pH of 0.6 M NH.CI solution? Discuss your results. (Ka of NH= 1.8 x 10) NH. + H,O+ H,0 +NH,
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Q: For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62.576 g,…
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Q: The Ksp of AgBr at 25°C is 5.0 x 10–13. a. Calculate the molar solubility of AgBr in pure water.…
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Q: 5.The solubility product, Ksp, of sparingly soluble salt with the formula M2X (where M ismonovalent)…
A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: 3. An EDTA solution is standardized against high purity CaCO3 by dissolving 0.3982 g CaCO3 in…
A: Given data,Mass of CaCO3=0.3982gVolume of EDTA=38.26mLpH=10.0
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Q: a.) What is the precipitation pH in gravimetric sulfate determination? Why is precipitation not done…
A: a) Sulfate is gravimetrically determined by using barium chloride solution.
Q: For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g,…
A: Moles of EDTA = Moles of Ca2+ in solution 23.6 mL of 0.0095 M EDTA solution was used Therefore,…
Q: a. Calculate the molar solubility of AgBr in pure water.Ksp for AgBr is 5.0×10-13. b. Calculate the…
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Q: 20. If 145 mL of a 0.0078 mol/L solution of CUNO3 was mixed with 195 mL of a 1.48 × 10-3 mol/L…
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Q: The solubility of Ba(OH)2 is 5.0 x 10-3 g/L a) Write a balanced equation for the solubility…
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: A 5.55-g sample of a weak acid with Ka = 1.3 * 10 - 4 was combined with 5.00 mL of 6.00 M NaOH, and…
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Q: For complexometric titration of Ca (II) ions in the shell of an egg sample weighing 59,427 g, the…
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Q: CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42-…
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Q: 4. A buffer was prepared using 10.0 mL of 1.90M HAc and 1.20 M NaAc (where Ac- is C2H3O2- ). The Ka…
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Q: The solubility of AgOH is 2 x 10-8 g/L a) Write a balanced equation for the solubility equilibrium…
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Q: Q1: A: Calculate the solubility product constant for PbCl2, if 80.0 mL of a saturated solution of…
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Q: A 41.00 mL mixture containing 0.0727 M Tl+ and 0.0727 M Hg22+ is titrated with 0.0867 M NaI…
A: Volume of the mixture = 41 mL Concentration of Tl+ = 0.0727 M Concentration of Hg+ = 0.0867 M
Q: A 1.250 g sample of cheese was subjected to KKjeldahl analysis to determine the amount of protein.…
A: Volume of HCl = 50 mL Molarity of HCl = 0.1050 M Volume of NaOH = 21.65 mL Molarity of…
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Q: 2. You are measuring the Fe(lI) content of a sample of FeCl2.4H20. You weighed out 1.20g FeCl2.4H20…
A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
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Q: What is the molar solubility of AgSCN in a solution that is buffered to pH 1.007 The Ksp of AgSCN is…
A: The solubility reaction of AgSCN can be written as, => AgSCN (s) -------> Ag+ (aq) + SCN- (aq)…
Q: A chemist wishes to prepare 121.00 mL of acetic acid/sodium acetate buffer solution with a pH of…
A: Given, A chemist wishes to prepare 121.00 mL of acetic acid/sodium acetate buffer solution with a…
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Q: A standard solution of EDTA is prepared, and by titration each ml is found to complex with the Mg in…
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Q: For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g,…
A: Molar ratio in which calcium ions bind EDTA is 1:1
Q: A 500 mL sample of a solution saturated at 25°C with calcium oxalate is evaporated to dryness,…
A: Equation involved:- Ca(C2O4)(s) = Ca2+(aq) + C2O42-(aq)
Q: If 145 mL of a 0.0078 mol/L solution of CuNO3 was mixed with 195 mL of a 1.48*10^-3 mol/L solution…
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Q: A: Calculate the solubility product constant for PbCl2, if 80.0 mL of a saturated solution of PbCl…
A: The solubility of a compound defines the dissolution of the compound in a given solution. The…
Q: :)An aqueous mixture that contains 0.100 M Ni²+ and 0.100 M Fe3+ is titrated with a 0.100 M CO;?-.…
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Q: A 0.3606-g of a weak monoprotic was dissolved in water and then titrated with 0.1040 N KOH solution.…
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Q: Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20…
A: Molar solubility of ions of LM2 and LQ = S Ksp of LM2 = 3.20 × 10-5
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Q: Sodium sulfate is slowly added to a solution containing (aq)0.0500 M Ca^2+(aq) and 0.0310 M Ag+(aq).…
A: Reactions that can take place are- Ca2+ (aq)+ SO42-(aq)→CaSO4 (s)2Ag+(aq) + SO42-(aq)→Ag2SO4 (s) Ksp…
Q: The solubility of Sr(OH)2 is 3.2 x 104 g/L a) Write a balanced equation for the solubility…
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: A 41.00 mL mixture containing 0.0727 M Tl+ and 0.0727 M Hg22+ is titrated with 0.0867 M NaI…
A: Volume of the mixture = 41 mL Concentration of Tl+ = 0.0727 M Concentration of Hg+ = 0.0867 M
Q: The solubility of Ca(OH)2 is 1.3 x 10-5 g/L a) Write a balanced equation for the solubility…
A: a) Calcium hydroxide dissociates into calcium ion and hydroxide anion as follows: Ca(OH)2 ⇔ Ca2+ +…
Q: For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g,…
A: At first we will determine the concentration of Ca2+ in the given 100mL solution. Then we'll extend…
Q: Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 ×…
A: Let the molar solubility of LM2 and LQ in water be s. Now find out the relation between the molar…
Q: The Ksp of AgBr at 25°C is 5.0 x 10-13. a. Calculate the molar solubility of AgBr in pure water. i.…
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Q: For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g,…
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Q: a) If the molar solubility of CaF2 at 35 °C is 1.24 x 103 mol>L, what is Ksp at this temperature?…
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- 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 9.14e-08 g of Sc(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Sc(OH)3.Ksp = (c) The Ksp of Cu3(PO4)2 at 25 oC is 1.40e-37. What is the molar solubility of Cu3(PO4)2?solubility = mol/LWill 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.(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
- If 145 mL of a 0.0078 mol/L solution of CuNO3 was mixed with 195 mL of a 1.48*10^-3 mol/L solution of KI, would precipitate form? Calculate the ion product (Q) for the potential precipitate. The ksp of CuI is 1*10^-12.Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?
- For µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µgThe sulfur content of insoluble sulfides that do not readilydissolve in acid can be measured by oxidation with Br2to SO42.25Metal ions are then replaced with Hby an ion-exchange column,and sulfate is precipitated as BaSO4with a known excess ofBaCl2. The excess Ba2is then titrated with EDTA to determinehow much was present. (To make the indicator end point clearer,a small, known quantity of Zn2also is added. The EDTA titratesboth the Ba2and the Zn2.) Knowing the excess Ba2, we cancalculate how much sulfur was in the original material. To analyzethe mineral sphalerite (ZnS, FM 97.46), 5.89 mg of powderedsolid were suspended in a mixture of CCl4and H2O containing1.5 mmol Br2. After 1 h at 20 C and 2 h at 50 C, the powder dis-solved and the solvent and excess Br2were removed by heating.The residue was dissolved in 3 mL of water and passed throughan ion-exchange column to replace Zn2with H. Then 5.000 mLof 0.014 63 M BaCl2were added to precipitate all sulfate as BaSO4.After the addition of…You are a CEM 262 TA and are preparing a 0.36 M ZnCl2 solution as an unknown for the EDTA titration experiment. The pH must be below what value to avoid precipitation of zinc hydroxide in the solution? The solubility product of Zn(OH)2 is 3×10-16. For this calculation, assume that the solution is ideal.
- You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mLUsing basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =123 mL of a 0.352 M Ca(NO3)2 solution is mixed with 251 mL of a 0.254 M solution of NaF at 25ºC. Calculate Qsp for the precipitate formed.