1- In the Group 2 precipitations, the Sulfide Ion (S) is generated in an Acidic environment. If the H;S concentration is maintained at 0.1M and the pH 1013 for H,S.). = 1, what is the [S] concentration? (K1 = 1 x 107 and Kn i %3D
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![1- In the Group 2 precipitations, the Sulfide Ion (S) is generated in an
Acidic environment. If the H,S concentration is maintained at 0.1M and
the pH = 1, what is the [S?] concentration? (K1 = 1 x 10 and Ka2 = 1 x
1013 for H2S.).
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- (a) Will Co(OH)2 precipitate from solution if the pH of a0.020 M solution of Co(NO3)2 is adjusted to 8.5? (b) WillAgIO3 precipitate when 20 mL of 0.010 M AgIO3 is mixedwith 10 mL of 0.015 M NaIO3? (Ksp of AgIO3 is 3.1 x 10-8.)Calculate the pH when 1.77 g of C6H5COONa (FW = 144.1 g/mol) is added to 48 mL of 0.50 M benzoic acid, C6H5COOH (FW = 122.1 g/mol). Ignore any changes in volume. The Ka value for C6H5COOH is 6.5 x 10^-5.The composition of PBS is 0.137M NaCl, 0.012M Phosphate, 0.0027M KCl, pH 7.4. Below is the protocol to make 1 litre of 10x concentrate PBS. Combine the following: • 80g NaCl • 2g KCl • 14.4g Na2HPO4 (dibasic anhydrous) • 2.4g KH2PO4 (monobasic anhydrous) • 800mL distilled H2O 1. Adjust pH to 7.4 with HCl 2. Add H2O to 1L 3. Autoclave for 20 minutes on liquid cycle. Store at room temperature. Which ions are being produced by this process, assuming that each of the chemical compounds dissociate into their constituent parts once they are dissolved in water?
- What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.Calculate the pH when 2.05 g of C6H5COONa (FW = 144.1 g/mol) is added to 44 mL of 0.50 M benzoic acid, C6H5COOH (FW = 122.1 g/mol). Ignore any changes in volume. The Ka value for C6H5COOH is 6.5 * 10^-5. Andv. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.
- 3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5 4. Give five (5) techniques on how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry. please answer all questions. I don't have questions left so i cannot repost the other questionA hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the Ksp values given in Appendix J.) (a) Hg22+ and Cu2+ (b) SO42− and Cl– (c) Hg2+ and Co2+ (d) Zn2+ and Sr2+ (e) Ba2+ and Mg2+ (f) CO32− and OH–
- A solution is made by dissolving 0.111 moles of N2H4 (Kb = 3.0 x 10-6 ) and 0.199 moles of N2H5Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 MUnlike propanoic acid, magnesium hydroxide, Mg(OH)2 does not dissolve well in water. The Ksp of Mg(OH)2 is only about 2 × 10–11. Yet, what will be the result if 75 mL of 0.0050 M Mg2+ are mixed together with 55 mL of 0.00010 M OH–? Write an appropriate expression (equation) for the Ksp of Mg(OH)2(s). Then, calculate Qsp and state accordingly whether a precipitate will form or not