Predict the solubility product constant: Ag2CO3(s) > 2Ag*(aq) + CO3-2(aq) Sample answer format: [Al+3][X-] *Put /or numbers outside the bracket if applicable
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![Predict the solubility product constant:
Ag2CO3(s) <> 2Ag* (aq) + CO3-2(aq)
Sample answer format: [Al+3][X-]
*Put / or numbers outside the bracket if applicable](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F26b75deb-dc7c-49f9-b302-4892147bba07%2F0bfe22c5-a63b-4e1d-b886-61b910975f15%2Fq7l1u4o_processed.jpeg&w=3840&q=75)
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- The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant. Determiner the ff. volume of NaOH used moles of OH- usedThe equilibrium constant for formation of CuCl2- is given by; Cu+(aq)+2Cl-(aq)→CCl2- β=7.9×104 What is the solubility of CuCl in the solutions having the following analytical NaCl concentrations: (a)5.0M (b) 5.0×10-2M (c)5.0×10-4M Please explain each and every concept and provide the right answer. Explain well answer fast as possible with good explanation
- Calculate the solubility at 25°C of AgBr in pure water and in 0.49M NaCN. You'll probably find some useful data in the ALEKS Data resource. ksp=5.35×10−13 Round your answer to 2 significant digits.Calculate the solubility of silver chromate in water: Ag2CrO4 ----------- 2Ag + + CrO42- Express the answer in g / 100 ml (in power form and with two decimal places) Ks (Ag2CrO4), 1’2 10-12(c) 1.0cm^3 0.25 moldm^-3 potassium chromate(VI), K2CrO4, is added as an indicator. At the end-point, all the silver chloride has been precipitated in the 52.5cm^3 solution. A slight excess of silver ions causes a red-brown precipitate of silver chromate(VI) to form. 2Ag + (aq) + CrO4 2- (aq) - - > Ag2CrO4 (s) (i) The solubility product of silver chloride is: Ksp = 2.0 ×10^-10 mol^2 dm^-6 Use this value to explain why [Ag+] = 1.41 × 10^-5 moldm^-3 at the end point.
- The solubility product constant of mercury(I) iodide is 1.2 × 10-28 at 25°C. Estimate the concentration of Hg22+ and I2 in equilibrium with solid Hg2I2.Solid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until the concentration of hydroxide ion is 0.0568 M. The percent of nickel ion remaining in solution is __ % Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2 2.5 ×…As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…
- Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a) [Ag][PO4] (b) [Ag+][PO43 - ] (c) [Ag+]3[PO43 - ](d) [Ag+[[PO43 - ]3 (e) [Ag+]3[PO43 - ]3A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show workYou 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 mL