Sn2 and N (starting concentration 10 mol/L) should be separated by fractionated precipitation using H₂S. Does a pH range exist allowing to completely precipitate one metal (i.e. the remaining concentration of the precipitated ion has to be 10 mol/L or less) whereas the other stays in solution at its initial concentration? Please calculate this pH range whereby pH values below zero are set to zero! Please illustrate the situation graphically by plotting pH versus in solution/precipitating/fully precipitated for the two ions (9) Solubility product (SnS): 10; (NIS): 1021; Acid constant (H2S): 10-20, r/Concentration of H2S in water: 0.1 mol/L
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- (f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)A buffer solution is made that is 0.355 M in HCN and 0.355 M in KCN. If K, for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH =| Write the net ionic equation for the reaction that occurs when 0.095 mol HNO, is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H;0* instead of Ht) A buffer solution is made that is 0.376 M in HCN and 0.376 M in NaCN. If K, for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.105 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +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/L
- In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H,O, at 20 – 25°C) co so Cro C,0; OH- Mg?+| 0.00069 0.18 35.7 54.8 0.038 Са2+ 0.16 0.00066 0.205 13.2 0.00061 Sr2+ 2.25 0.00034 0.135 0.106 0.005 Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075 For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate. Mg(NO,), and (NH,),CO, : MGCO, Incorrect ВаCl, and NaОН: Ba(ОН), Incorrect AgNO, and NaBr : AgBr Ca(NO,), and KCI : СаCl Incorrect SDECIAI ASO 1..A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10Consider a flask containing 25.00 mL of 0.100M sodium benzoate (NaC, H5C00). This is titrated with a 0.110 M nitric acid solution from a burette. Given: K, of C,H;co0" is 1.6 x 10-10. Determine the pH of the solution in the flask after 32.00 mL of the acid has been added? You must show any reaction equation(s) that you may think are necessary. Determine the pH of the solution in the flask at the half-way point of the titration.
- Please help me...... a. Do you expect the pH at the equivalence to be lowest when a 0.0500 M (CH3)3N(aq) solution or a C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution at 25.0 oC? Motivate your answer! (CH3)3N (Kb = 6.5 × 10-5) and C5H5N (Kb = 1.7×10-9) are weak monoprotic bases. Calculate the pH at the equivalence point and 25 oC when 1.00 L of a 0.0500 M C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution. Calculate the molar solubility for CaCO3 in a 0.060 M Ca(NO3)2(aq) solution. Ksp= 3.1 × 10-9 for CaCO3.An analyst was titrating a solution of unknown acetic acid concentration with 0.01 M NaOH using phenolphthalein as indicator. After adding exactly 39.4 ml of the titrant drop-wise, the analyte solution started to turn light pink. The titrant volume 39.4 ml is best referred to as the O equivalence point. Onone of the choices O standardization point. O equilibrium point. O endpoint.A chemistry graduate student Is glven 300. mL of a 1.50M trimethylamine ((CH, N solutlon. Trimethylamine Is a weak base with K,=7.4x 10 ". what 3. mass of (CH,NHBr should the student dissolve in the (CH, N solutlon to turn It Into a buffer with pH = 11.107 (CH), 3 You may assume that the volume of the solution doesn't change when the (CH,) NHBR Is dissolved In it. Be sure your answer has a unit symbol, and round It 3 to 2 significant digits. do Ar x10 Check Explanation 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility V I 3:55 hp 火 Ce & esc $4 8. #3 ! 4 3 t y r e W
- In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.31 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.98 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker. After 22.04 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution? Report your answer with 3 sig figsChoose the acid below that would make the most effective buffer for a solution to maintain a pH of 5.00 (aq., 25 oC), given a 0.500 M concentration of it and its conjugate salt. a) propionic acid, Ka = 1.34 x 10–5 b) HN3, Ka = 1.90 x 10–5 c) butanoic acid, Ka = 1.52 x 10–5 d) NH4Cl, Ka = 5.56 x 10–10 e) benzoic acid, Ka = 6.30 x 10–5