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1. A solution is prepared that initially contains 0.10 M Ag+(aq) and 0.80 M NH3 (aq).
a) The Kf for the formation of Ag(NH3)2+(aq) is 1.7 x 10^7. Write the equilibrium equation that represents the formation of this complex ion.
b) Calculate the [Ag+] at equilibrium.
c) Solid NaCl is added to the solution until the chloride concentration reached 0.010 M. Would the precipitate AgCl form? Justify your answer using a calculation. (Ksp of AgCl is 1.8 x 10^-10).
A nitric acid solution containing 71.0% HN)3 (by mass) has a density of 1.42 g/mL. How many moles of HNO3 are present in 1.00L of this solution?
By substituting two hydrogen atoms on the benzene ring with methyl groups, write line-angle formulas of all constitutional isomers. Name each isomer.
Selective precipitation, fractional precipitation, amphoteric precipitate solubilization, competitive equilibrium solubilization: anion protonation, competitive equilibrium solubilization
The compound malonate is an analog of succinate and is a strong inhibitor of succinate dehydrogenase. The active site of the enzyme will bind to either molecule, however malonate will not undergo any reaction and gets stuck on the enzyme.
A proton in a linear accelerator has a de Broglie wavelength of 143 pm. What is the speed of the proton?
A steel cylinder contains 120. moles of nitrogen gas at a temperature of 32 C and pressure of 775 torr. After some of the nitrogen gas has been used,
Single double triple bonding, Explain the characteristics of a single, double, and triple bonds including why they form and how the electrons
How many grams of NaOH are needed to neutralize 20.0 mL of 0.150 M H2SO4 solution? (b) How many liters of 0.500 M HCl(aq) are needed to react completely with 0.100 mol of Pb(NO3)2(aq)
What substances are present after the reaction is over? (Hint: Write a balanced chemical equation for the reaction first.) How many grams of water are formed?
The solutions mixed together are 53.6 mL of 0.129 M hydrochloric acid, 104.1 mL of 0.215 M of nitric acid, 501.5 mL of 0.0126 M calcium hydroxide, and 201.0 mL of 0.122 M rubidium hydroxide. Did the acids and bases exactly neutralize each other?
Calculate the pH at each of the following points in the titration of 50 mL of 0.2000M acetic acid using 0.222M NaOH. Ka= 1.8 x 10^-5 (show work)
In the titration of a solution of a weak monoprotic acid with a .1325M solution of of NaOH, the pH was halfway to the equivalence point was 4.42.
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