8. Calculate the equilibrium concentration of each aqueous species (H2A, HA– A2–, H3O+, and OH–) in the solution. Assume a temperature of 25°C. H2A: pKa1 = 2.05 and pKa2 = 6.22 a. 0.10 M H2A b. 0.10 M Na2A
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8. Calculate the equilibrium concentration of each aqueous species (H2A, HA– A2–, H3O+, and OH–) in the solution. Assume a temperature of 25°C. H2A: pKa1 = 2.05 and pKa2 = 6.22
a. 0.10 M H2A
b. 0.10 M Na2A
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- 0.0500 M HF (Ka= 7.20 x 10–4) determine the equilibrium molar concentration of H3O+ and equilibrium molar concentration of HF (in 3 sig. figures).A solution is 0.010 M in HCl and 0.010 M in NH4Cl. What is the molar concentration of NH3 at equilibrium? Kb(NH3) = 1.8 x 10-510.5 mL of 0.139 M Mg(NO3)2 is mixed with 11.9 mL of 0.625 M NaOH. Calculate the final concentration (in M) of hydroxide ion ([OH-]) after any reaction that occurs goes to completion
- Which of the following is TRUE about the RbCl salt? I. RbCl ions do not participate in hydrolysis with water. II. RbCl are derived from weak base and weak acid respectively. III. RbCl has a value of Ka = Kb. IV. RbCl solution is acidic. Consider the reaction: 2 SO2 (g) + O2(g) ⇄ 2 SO3(g); ΔHo = -198.2 kJ/mole Predict the shift of the chemical reaction in the given system if the pressure of the gas system was increased. The equilibrium shifts in the forward direction. The equilibrium shifts in the reverse direction. Equilibrium is not changed or affected.1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?ICE for each addition of common ions AgCl, Ag2So4ksp of AgCl = 1.77 x 10^-10 Concentration of Ag= 0.0304380 Concentration of Cl- = 5.81510x10^-9 concentration of SO42- = 0.0152190
- Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml…Assume the following process is at equilibrium.NaCl(s) <----->Na+(aq) + Cl–(aq) deltaH0> 0How will the following changes influence this equilibrium? Indicate whether each change will cause additional NaCl to dissolve, will cause NaCl to precipitate, or will have no influence on the equilibrium.__________ (a) The temperature is increased.__________ (b) The pH is decreased.__________ (c) MgCl2 is added to the reaction vessel.What is the equilibrium concentration of H2C2O4 in a 0.542 M oxalic acid, H2C2O4, solution? For oxalic acid, Ka1 = 6.1 x 10–2 and Ka2 = 5.1 x 10–5. a. 1.4 x 10–1 M b. 1.1 x 10–1 M c. 2.3 x 10–1 M d. 3.88 x 10–1 M e. 8.9 x 10–2 M
- In which of the following solutions is FeS most soluble? K2S (NH4)2Fe(SO4)2(H2O)6 Fe(NO3)2 KNO3Calculate how much lithium bromide (s) would have to be dissolved in DI water in order to make 1.00 mL of a saturated lithium bromide (aq) solution if this salt has a solubility of 286 g/L at 25°C.What is the pH (to two decimal places) of a saturated aqueous solution of LiF (at 25 °C)? Ksp = 3.8 × 10–3; Ka(HF) = 6.67 × 10–4