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A: Equilibrium constant (Kc) is a characteristic constant of any specific reversible reaction. The…
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A: The reasons for using 6M NH3 and not 6M NaOH solution when separation Fe3+ and Al3+ ions from Ca2+,…
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Q: In gravimetric analysis, precipitation is a quantitative method commonly used. However, its efficacy…
A: The answer is given below
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A: Given mass of NOCl = 1.5 g percentage dissociation = 57.2℅
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A: Ca3(PO4)2 dissolved readily in acidic medium Ca3(PO4)2 -----> 3Ca2+(aq.) + 3PO43- In acidic…
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A: Given: 0.050M KNO3 To find: activity coefficient of K+.
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Q: Describe the common-ion effect?
A: The common ion effect has to be described.
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A: Hume-Rothery Rules is Related with the condition that determine whether an alloy or impurity element…
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A: One mass balance is simply written as, Na+ = 0.1MIf acetate does not react further,CH3COO- =0.1M
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A: Given: Volume of solution = 250 mL. And concentration of cadmium ion = 100 ppb.
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Q: Calculate the activity coefficient of K+ in 0.050 M KNO3.
A:
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Q: 10.) Calculate the activity coefficient of K* in 0.050 M KNO3.
A:
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A: Solubility is a phenomenon where the solute get dissolved in a solvent to form a solution. The…
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A: According to Henry’s law, the solubility of a gas is expressed as S = KP where S is the solubility,…
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A: The purpose of adding an excess of the precipitating agent is given below.
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A: Here we have to mention the solvents to dissolve AgCl, Hg2Cl2 and PbCl2 precipitates-
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Q: In the experimental procedure, it is instructed to cover the vessel containing the saturated…
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Q: Explain the common-ion effect.
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Q: For ferrous hydroxide, Fe(OH)2, KSP = 1.4x10-15, corresponding to a solubility of about 0.6 mg/L.…
A: Ksp is known as the solubility product constant and is equal to the equilibrium constant for a…
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A: Answer :- In acidic solution, calcium phosphate, Ca3(PO4)2 is readily soluble than calcium sulfate,…
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- Will silver iodide precipitate from a solution that is 0.0045 M AgNO3, 0.15 M NaI, and 0.20 M KCN?NEED HELP PLEASE GRAVIMETRIC ANALYSIS (Exercises) Instructions: Answer each of the problems below by showing your solutions neatly and logically. You may use periodic table for atomic masses of elements. Copy and answer each problem and please box your final answers. 9. What weight of pyrite ore (impure FeS2) must be taken for analysis so that the BaSO4 precipitate weight obtained will be equal to one-half that of the percent S in the sample? NOTE: KINDLY WRITE THE SOLUTIONS ON A SEPARATE SHEET OF PAPERNeutralization experiment/ Titration of KHP Sample 1 Sample 2 Mass of flask and KHP 43.07 g 42.77 g Mass of empty flask 42.05 g 41.09 g Mass of KHP 1.02g 1.68g Final buret reading 8.95 mL 22.66 mL Initial buret reading .98 mL 8.95 mL Volume of base used 7.97ml 13.71 1)Moles of base (NaOH) used to neutralize the acid above. 2)Molarity of base (NaOH). 3) Average Molarity of base please show step by step. Thank you
- Lead(II) arsenate, Pb3(AsO4)2, has been used as an insecticide. It is only slightly soluble in water. If the solubility is 3.0 105 g/L, what is the solubility product constant? Assume that the solubility equilibrium is the only important one.The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a Which beaker on the right, X or Y, depicts the solution after the addition of two formula units of NaOH? b How many HCl molecules can be added to the original buffer solution before the buffer capacity is exceeded? c Draw a picture of the solution where the buffer capacity has been exceeded by the addition of HCl.A solution of 0.00016 M lead(II) nitrate, Pb(NO3)2, was poured into 456 mL of 0.00023 M sodium sulfate, Na2SO4. Would a precipitate of lead(II) sulfate, PbSO4, be expected to form if 255 mL of the lead nitrate solution were added?
- In an experiment, a solution of AgNO3 was added to known solutions of NaCl, NaBr, and NaI and each reaction formed a precipitate. When chlorine water and hexane were added to these known samples, the hexane layer showed no color for NaCl, turned orange for NaBr, and turned purple for NaI. The observations for your unknown are listed below. Which ion is your unknown? UNKNOWN # 98 Experiment Observations TEST 1 Add AgNO3 Off-white ppt TEST 2 Add BaCl2 reaction does not occur TEST 3 Add dilute HCl reaction does not occur TEST 4 Add chlorine water & hexane orange top layer Group of answer choices chloride bromide iodide none of the aboveThe Kspvalue for lead chromate, PbCrO4, is 2.01016at 25 °C. Calculate its solubility at 25 °C.A sample of sodium chloride, NaCl, weighing 0. 0678 g is placed in a 25.0-mL volumetric flask. Enough water is added to dissolve the NaCl, and then the flask is filled to the mark with water and carefully shaken to mix the contents. What is the molarity of the resulting solution?
- Consider the equilibrium reaction: AX3(s) ⇌ A3+(aq) + 3X-(aq). What is the solubility of AX3 (MM = 78.0g/mol) in mg/L at 250C if its Ksp is 1.0 x 10−33? answer: 1.92x10-4 mg/LExperiment4: Solubility Product In the experiment to determine the solubility of KI04, in water, the following observations are made at a certain temperature: Volume of saturated KI04 solution taken in the conical flask = 25.0 mL KI added=2g H2SO4 (3.0 M ) added = 20.0 mL. Volume of 0.200M sodium thiosulphate used for titration = 8.00 mL Q1.If the mean ionic activity coefficient, γ± of KIO4 in the saturated solution is 0.85, what is Ksp of KIO4.?Exercise 15.8 When aqueous solutions of Na2SO3 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M NaSO4 are mixed.