SPECTROPHOTOMETRIC DETERMINATION OF A SOLUBILITY PRODUCT CONSTANT LAB 3. The PH of a saturated Mg(OH)2 solution is 10.46. A) Calculate the [OH-1] in the solution. Show the calculation. B) Calculate the [Mg+2] in the solution. Show the calculation. C) Calculate the Ksp of Mg(OH)2.
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SPECTROPHOTOMETRIC DETERMINATION OF A SOLUBILITY PRODUCT CONSTANT LAB
3. The PH of a saturated Mg(OH)2 solution is 10.46.
A) Calculate the [OH-1] in the solution. Show the calculation.
B) Calculate the [Mg+2] in the solution. Show the calculation.
C) Calculate the Ksp of Mg(OH)2.
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- Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).The solubility product constant for Hg(IO3)2 is 3.2 x 10-13. What is the Hg2+ concentration of a solution prepared by mixing 50.0 mL of 0.200 M Hg (NO3)2 with a) 50.0 mL of 0.05 M KIO3 ? b) 50.0 mL of 0.4 M KIO3 ? c) 50.0 mL of 0.5 M KIO3 ?A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 ml ot a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONA). [Ka= 1.8 x 10-1 What is the new concentration of the conjugate base, CH3COO after buffering? 0.3385 0.2434 0.1172 0.2269 0.4287
- If a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].Q:3-2 How many moles of NH,CI must be added to 2.0 L of 0.1M NH3 to form a buffer whose PH of 9.00 ? (assume that the addition of NH,CI does not change the volume of the solution. For NH3 kb= 1.8 X 10-3, pkb= 4.75) Q:3-3 How many moles of NH,CI must be added to 2.0 L of 0.1M NH3 to form a buffer whose PH of 9.00 ? (assume that the addition of NH,CI does not change the volume of the solution. For NH, kb= 1.8 X 10-3, pkb= 4.75)What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in sodium lactate [CH3CH(OH)COONa or NaC3H5O3]? For lactic acid, Ka = 1.4 * 10-4.
- Answer using this data for the remaining questions on this page: For 1.0L of an acetic acid solution: Ka = 1.8 x 10-5 and [HA] = 0.250M 2. Calculate the pH of the solution. 3. What is the pka? 4. Calculate the pH of the solution if you make it a buffer by adding enough solid sodium acetate to make the concentration of acetate ion equal to 0.35M. The volume of the solution does not change. 5. What is the new concentration of [HA] if 2.0mL of 5.00M of HCI is added to 1.000L of the solution above? 6. What is the new pH?Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable? (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base) (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base) (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base) (D) Any of themIn 6.0 M NaOH, M(OH)3 has a solubility of 1.0M due to the formation of the [M(OH)4]¯ ion. Calculate the Ksp of M(OH)3. [M(OH)4]¯: Kf = 1.0 × 1010). %3D ds,
- 7. Refer to the following table: Table 2-2. Change in pH of 0.2 M Acetate Buffer after addition of Acid or Base [Base]:[Acid] 0.005:0.195 Addition pH HC1 0.095 mol 3.1 HC1 0.075 0.025:0.175 3.9 HС1 0.05 НС1 0.025 0.05:0.15 4.2 0.075:0.125 4.5 0.1:0.1 0.125:0.075 4.7 NaOH 0.025 mol 4.9 NaOH 0.05 mol 0.15:0.05 5.2 NaOH 0.75 mol 0.175:0.025 5.5 NaOH 0.095 mol 0.195:0.005 6.3 a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-' acetic acid and 0.1 mol L-1 sodium acetate), given that the pKa of acetic acid is 4.7. b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L1 acetate buffer? c. Compare the pH value in (b) with that obtained after adding 0.05 mol NAOH to 1 L of water (a simple solution of 0.05 mol L-' NaOH). d. How much acid or base can be added to 1 L of the 0.2 M acetate buffer so that the pH does not change appreciably (i.e., what is its buffer range)?For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 2 pH = 3 pH = 5 O yes BaCO, dlo O no O yes Cal, O no O yes Ni(OH), O no Check Terms of Use Privacy Explanation 2021 McGraw-Hill Education. All R V 1 10: Ocer24) The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a solution with a pH of 10.6. (aq., 20 °C). A) 2.5 × 103 В) 3.9 х 10-4 C) 7.7 × 10- 13 D) 3.2 × 10-10 E) 5.0 × 10-17 F) 2.1 × 104 G) 5.0 x 10-12