A 30 cm'aliquot of 0.075 M Sodium hydroxide (NaOH) is titrated against a standardised HCl solution of concentration 0.090 M. What is the pH after 0.1 cm' of HCl excess (i.e. V at equivalence + 0.1)? O 5.04 8.95 7.00 10.21 3.79
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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).Calculate the pH of a titration mixture when 25.36 mL of 0.081 M NaOH has been added to a 50.00 mL sample of 0.0950 M CH₂COOH (K, (CH₂COOH) = 1.8 x 10-5 Enter the pH to two decimal places, i.e., 1.23, do not include units2. 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 a
- Calculate the molar solubility of lead(II) iodide in water at 25°C. given that Ksp = 7.1 x 10-9Calculate the molar solubility of Mg(OH)2 (Ksp = 1.8 * 10-11 ) in(a) pure water;(b) 0.0862 M MgCl2.(c) 0.0355 M KOH(aq).3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) is precipitated as BaCO3 by passing through Ba (OH) 2 solution. The excess of the base is titrated with 23.6 mL 0.0108 M HCl in addition to the phenol phthalate (f.f.) indicator. Calculate the CO2 concentration in this air sample in ppm. (Take the density of CO2 as 1.98 g / L. C = 12, O = 16 g / mol).1: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中
- 2. In the titration of 50 ml. of 0.05 M of AGNO; solution with 0.05 M KSCN solution, calculate the molar concentration of Ag* in the conical flask solution after the following additions of titrant KSCN solution (Kp - [Ag*|[SCN]- 1.0 X 10-12): (a) 25 mlL (b) at equivalent point (c) 55 mL9. Calculate the pH of 0.250 L of 0.36 M formic acid (CH2O2) – 0.30 M sodium formate (CHOżNa) buffer. The Ka for formic acid is 1.8 x 104. CH2O2 (aq) H20 (1) сно? (ag) + Hзо" (аq) + a. Calculate the pH of the above buffer after 0.0050 mol of NaOH have been added. Assume that the volume remains constant. b. Calculate the pH of the buffer after 0.0050 mol of HCI have been added to the original buffer (top of page). Assume that the volume remains constant.What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of 4.00? Report to 3 sig figs
- Ksp for AgCl is 1.77E-10. What is the molar solubility of AgCl in a solution of 0.36 M NaCl?Include at least 3 significant figures in your answer.to ritwong art insvang of twol 10 8.0 2. Using the attached table, calculate the molar solubility of BaSO4 in a. Pure water dissociation ea = = US = 1.07 × 10-10 nistdo of bean Doy +2 BaSO₁. Ba² + Sou aq 3 S 31.07x10 071 S=(2.1615 × 10-1) (b. In a 2.00 M sodium sulfate solution x +2 13 И -4 a4 1/2 N 2.99x10 Basou +2Nasoy Ba² + 2 Na + 3504 017 M Noa) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most