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Approximate the heat of reaction for the following equation using thermodynamic tables: CuO (s) + AgNO3 (aq) Cu(NO3)2 (aq) + Ag2O (s)
Calculate the pH at the equivalence point in titrating 0.120 M solutions of each of the following with 8.0×10?2 M NaOH. -benzoic acid (C6H5COOH)
The density of a given solid and liquid of molar mass 147.2 g/mol at its normal melting temperature of 372.54 K are 992.6 Kg m-3 and 933.4 Kg m-3, respectively. If the pressure is increased to 120 b
Calculate the fraction of lidocaine present in the form LH . MOPS Buffer Ka = 6.3 × 10-8. Lidocaine Kb = 8.7 × 10-7
The Ka of Hypochlorous, HClO acid is 3.5x10^-8. Calculate the ph of a solution at 25 C that is .005 M in HClO
Calculate Ka for propionic acid (HC3H5O2) if a 500 mL solution of propionic acid containing 9.250 g of the acid has a pH of 2.71
Calculate the temperature of boiling water at an elevation of 6000ft (2000m) given that the atmospheric pressure is 0.8atm. Assume delta H_vap is independent of T.
The pH in a 0.25 M solution of the acid HBrO is 4.65. Using this, calculate the value of Ka for the acid HBrO.
If an 20 mL acetic acid is neutralized with 50 mL of 0.8 M NaOH, what is the concentration of the acid
Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOH required for precipitation to begin in 2.8*10^-3 M Fe(NO3)2
When 85.00 mL of 0.250 M Ca(OH)2 (aq) and 15.00 mL of 0.750 M Pb(NO3) (aq) are mixed together in a beaker a yellow precipitate is formed. Assume all heavy metal hydroxides are insoluable
Calculate the ratio of NaF to HF required to create a buffer with pH = 4.10. Calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH = 10.22
Solve an equilibrium problem (using an ICE table) to calculate the pH 1)a solution that is 0.13M in NH3 and 0.15M in NH4Cl 2) 185.0 mL of 0.12M C2H5NH2 with 265 mL of 0.20M C2H5NH3Cl
A solution is made that is 1.1×10^?3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains
Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOH required for precipitation to begin in each case. A - 2.8*10
Consider a solution that is 1.1*10^-2 M in Ba2+ and 2.0*10^-2 M in Ca2+. A - If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which
What is the pH at the equivalence point in the titration of 25.00 mL of 0.020 M NH3 with 0.015 M HBr? Kb for NH3 = 1.8 x 10^-5
Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOH required for precipitation to begin in each case. A - 1.4*10
Compare and contrast these methods of extraction- Solid phase extraction, liquid liquid extraction, Supercritical fluid extraction, Derivatization, and solid-phase microextraction
Calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.180 M NaOH solution? Express your answer numerically to three significant figures.
If the system is allowed to expand as N2 is added at a cosntant total pressure of 1 bar, what will be the equilibrium degree of dissociation when the N2 partial pressure is 0.6 bar
The stock solution of KMnO_4 has a concentration of 2.6 X 10 ^ -4M. The pipette has a volume of 10.0mL. What is the amount of KMnO_4 delivered to the solution, in moles
The movie has been moved to the position where about half of the F^2+ solution has been added. At this stage, what quantity of Fe^2+, in moles have been added to the beaker for each mole of MnO
What ions are in these solutions. cold tap water, 0,9 % NaCl (aq), 0,1 M acetic acid, 0,1 M HCl, 0,1 M NaC2H3O2 (aq), 0,1 M ammonia.
Which of the molecules N2, NO, O2, C2, F2, and CN would you expect to be stabilized by (a) the addition of an electron to form the anion (b) the removal of an electron to form the cation