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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- Calculate the minimum mass (g) of KOH that would have to be added to the initial buffer in Problem-Solving Example 15.5 to exceed its buffer capacity.Predict the solubility product constant: Ca3(PO4)2(s) + 3Ca*2(aq) + 2PO4-3(aq) Sample answer format: [Al+3][X-] *Put / or numbers outside the bracket if applicable5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)
- A student is calculating the concentration of her standard solutions in order to create the calibration curve (standard curve). Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FeNCS²+]eq, for a solution created by combining 2.00 mL of 0.183 M Fe3+ (aq) with 225μL of 0.00199 MSCN- (aq). Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). You may assume that the volumes of these dilute, aqueous solutions are additive.Do the argentometric titration according to given data and fill in the blanks. Ag+ (aq) + Cl- (aq) → AgCl (s) (White) NaCl » Na* + Cl- SET 2 Measured Weight of NaCl, (gr) 2.5 g Measured Weight of Cl- , (g) Volume of Stock Solution, (mL) 200 mL Amount of Sample taken from the stock solution, (mL) 9mL Normality of AgNO3, (N) 0.1 N Initial burette reading, (mL) O mL Final burette reading, (ml) 6.85 mL Volume of AgNO; Consumed, (mL) 6.85 mL Amount of AGNO3 Consumed, (mg) Calculated Weight of NaCI in stock Solution, (g) Calculated Weight of CI- in stock Solution, (g) Error in Calculating Amount of CI-(%)A completely made up compound of fluoride, XC12, is found to have a molar solubility of 8.31 x 10-23, when dissolved in an 2.43 M AICI3 (aq) solution. What is the Ken for this compound? Please input your answer to the second decimal place. Type your answer.
- Consider the equilibrium shown. SrF, (s) = Sr + (aq) + 2F (aq) K = 2.60 x 10-9 Determine the concentrations of Sr+ and F in a saturated solution of SrF, in pure water (assume u = 0M). !3! [S?*1 = M [F] = Determine the concentrations of Sr+ and F in a saturated solution of SrF, in a solution with an ionic strength of 0.010 M. [Sr*] = [F] = MWhat is the molar solubility of a hypothetical compound AB in a solution containing 0.22 M B- given a K5, = 5.5 x 10-2? AB(s) = A*(aq) + B(aq) Add your answerWhat is the molar concentration of Ag+ when an excess of solid Ag2SO4 is added to 0.1063 M Na2SO4 so that some solid remains? The solubility reaction isAg2SO4(s) ↔2Ag+(aq) + SO42-(aq) Ksp = 1.20e-5
- 2. A buffer is made up of 345 mL each of 0.200 M CH3CO₂H and 0.135 M NaCH3CO2. Assuming that volumes are additive, calculate the pH of the buffer. The Ka of acetic acid is 1.8 x 10-5. CH,CO,H(aq) + H,O(!) = H,O*(aq) + CH,CO,(aq) K₂ = 1.8 × 10-5 aA titration of 29.2 mL of a solution of the weak base aniline, C@HNH, ( K 4.0 x 10-10), requires 21.61 mL of 0.155 M HCl to reach the equivalence point. CH_NHz(aq) + HyO* (aq) + C,H,NH, (aq)+H,O(l) a What was the concentration of aniline in the original solution? Concentration 0115 ✔ M The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus, [C,HNH] [H₂O+] [OH-]- = 0.155 mol HC1 1.00 L 1 29.2 mL b What are the concentrations of H₂O¹, OH, and C6H5NHs at the equivalence point? M C = 0.115 M x 21.61 ml x M Correct 1 mol C, H, NH, 1 mol HCl Show HintA solution contains 2.0 x10-4 M Ag+(aq) and1.5 x 10-3 M Pb2 + (aq). If NaI is added , wi l l AgI(Ksp = 8.3 x10-17)or PbI2 (Ksp = 7.9x 10-9) precipitatefirst? Specify the concentration of I-(aq) needed to beginprecipitation.SEE MORE QUESTIONS