Q: Write the dissolution reaction of sodium carbonate, of Ag2CrO4 and KMNO4.
A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…
Q: Consider the sparingly soluble salt silver oxalate, Ag,C2O4. Assume a solution temperature of 25°C…
A: a) Let the molar solubility of Ag2C2O4 is s mol/L The Ksp of silver oxalate, Ag2C2O4 is 5.47 x 10-12…
Q: ST5G.2 - Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.701 molar…
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Q: Calculate the solubility of lead iodate (Pb(IO3)2, Ksp = 3.68 x 10-13).... (a) ... in pure water…
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Q: A measure of the difference in solubility of the components of a mixture in two phases *
A: Answer - the partition-coefficient This is a measure of the difference in solubility of the…
Q: Explain why 6M NH3 and not 6M NaOH solution is used when separation Fe3+ and Al3+ ions from Ca2+,…
A: The reasons for using 6M NH3 and not 6M NaOH solution when separation Fe3+ and Al3+ ions from Ca2+,…
Q: The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the…
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Q: In gravimetric analysis, precipitation is a quantitative method commonly used. However, its efficacy…
A: The answer is given below
Q: How selective precipitation and simultaneous equilibria are used to separate ions
A: To find: How selective precipitation and simultaneous equilibria are used to separate ions
Q: describe how you can prepare 500mL of 0.10 M Fe2O3 (159.69g/mol) from the primary-standard-grade…
A: Calculate the number of moles of Fe2O3: 1 mL = 0.001 L
Q: Calculate the masses of (i) Ca(NO3)2 and, separately, (ii) NaCl to add to a 0.150 mol kg−1 solution…
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Q: What is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Ksp of AgCI…
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Q: (c) (a) Pure Pure Composition reactants products For the three curves, what is the common feature of…
A: The given graph is represented as follows:
Q: Describe the common-ion effect?
A: The common ion effect has to be described.
Q: Calculate the % relative error in solubility by using concentrations instead of activities for…
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Q: You have a solution that contains acetic acid, (CH3COOH or HAc). The concentration of acetic acid in…
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Q: The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid…
A: a) The dissociation vapor of NH4Cl at 427oC is 608kPa and at 459oC is 1115 kPa. The balanced…
Q: The concentration of a pure solid is left out of a equilibrium constant expression but a pure liquid…
A: Equilibrium constant expression : Keq = [products ] /[reactants]
Q: Calculate the % relative error in solubility by using concentrations instead of activities for…
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Q: For a titration to be effective, the reaction must be rapid and the yield of the reaction must…
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Q: Explain why buffer potential is maximised at the pH that matches the pka of the weak acid of the…
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Q: Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed…
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Q: For the reaction - H2 (g) + I2 (s) = HI (g) at 25°C and 1 atm, the equilibrium mixture contained 39%…
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Q: Estimate the pH of a solution of 0.50 M HCI(aq), assuming ideal behaviour. The mean activity…
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Q: Calculate the value of the reaction quotient, Q, of silver iodate (AgIO3) when 10.0 mL of 0.011 M…
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Q: What would be the KPs value of Al(OH)3, considering that its solubility is 2,5 x 10^-8 mol/L?
A: Given: Molar solubility of Al(OH)3 = 2.5 X 10-8 M.
Q: Write the relevant chemical reaction and mass-balance expression for 0.1 M NaCl.
A: Ans : Mass balance Reaction : Nacl (s) → Na+(aq) + Cl-(aq) To following the…
Q: the solubility of Ba(IO3)2 in a solution prepared by mixing 300 mL of 0.010 M Ba(NO3)2 with 200 mL…
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Q: Write the expression for the solubility-product constant for CaF2, and look up the corresponding Ksp…
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Q: If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,050…
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Q: Consider the reaction CaCl2 (s) = Ca2+ (g) + 2Cl- (aq) (Ksp = 5.5 x 10-6) 1. What is the solubility…
A: CaCl2 (s) = Ca2+ (g) + 2Cl- Solubility (mol/L):…
Q: What is the pH at 25 degrees Celsius of a saturated solution of magnesium hydroxide (the active…
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A: Given that: % of Fe3O4= mass (g) of Fe2O3×100 % To find: The total weight of magnetite?
Q: Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the…
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Q: The aluminum in a 1.200 g sample of impure ammonium aluminum sulfate was precipitated with aqueous…
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Q: Explain the common-ion effect.
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Q: Sn(OH), 48 = 5.45 x 10-27 CUCN K,= S =3.47 x 10- MgF; = 45- 5.16 x 10-1 NICO, K„ = s² = 1.42 × 10-7…
A: Given Substance KspSn(OH)2 Ksp = 4S3 = 5.45×10-27CuCN Ksp = S2 = 3.47…
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Q: 4. Phosphate is precipitated from its solution with ammonium molybdate, as (NH4)a[PMO12O40 XH20].…
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Explain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context of a titration.
Titration is used Redox reaction and Acid-Base reaction. There are 2 important stages of the reaction –
- Stoichiometric or equivalence point
- Endpoint
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- A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedA1) Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.156 molar CaCl2(aq). A2) Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.831 molar AlF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.]Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .
- A sparingly soluble salt silver phosphate, Ag3PO4, is in equilibrium with its ions in solution according to the following equation A93PO4(s) = 3 Ag*(aq) + PO (aq) Write an expression for Ksp of Ag;PO4 The solubility of silver phosphate, Ag;PO4, at 25°C is 1.59 x 10 mol/L. What is the Ksp for the silver phosphate at 25°C?For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?
- What is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Kgp of AGCI = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70×107? Express your answer in decimal notation rounded to three significant figures.Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case where the acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point, mol acid = mol base %3D At all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (and there is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can do them- a lot of them! One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions: [strong acid] = [H*] and pH = -log[H"] Something similar happens for strong bases. 1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Show all your work for each calculation (including the volumes for which the pH is given).…(a) Define and write the expression of Kw for the dissociation of water (H2O). Kw is the ________________ _____________ of ______________ (b) Calculate the pH of 0.1mol dm-3 potassium hydroxide (KOH(aq)) pH = C) Explain briefly the effect of temperature on Kw.
- The reaction of ozone in the atmosphere and nitric oxide has a reaction enthalpy and reaction entropy of -199 kJ mol-1 and -4.1 J K-1 mol-1, respectively. What is its reaction Gibbs energy at 25 °C? O3(g) + NO(g) → NO2(g) + O2(g) 1220 kJ mol-1 -200 kJ mol-1 -1420 kJ mol-1 -198 kJ mol-1Calculate the molar solubility of lithium phosphate, Li;PO4, given that the Kp of lithium phosphate is 2.37 x 10-11.The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.