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Problem- The solubility of slaked lime, Ca(OH)2 in water is 0.185 g /100ml. what volume of 0.00400 M HCl is needed to neutralize 14.0 ml of saturated Ca(OH)2 solution?
Solve the above problem and provide steps with explanation
What mass of ammonium chloride should be added to 2.45L of a 0.145M NH3 in order to obtain a buffer with a pH of 9.45
Calculate the mixing ratio (ppbv) of NO2. Assume T=20 degrees Celsius = 293 K; P = Atmospheric pressure. MW of NO2 = 44g/mol.
What is the final temperature (in oC) of a 37.6 g sample of graphite (specific heat = 0.720 J/(g K)) which absorbs 9.82 kJ of heat when it warms from 12.56oC
The reaction of bromine with acetone follows first order kinetics, i.e where k is the rate constant, c is the concentration at time t and c0 is the initial concentration.
calculate the equilibrium constant for the neutralization reaction. To calculate the equilibrium constant, you may find it helpful to represent the neutralization reaction as the sum of two separate reactions. (b) Calculate the pH, [CH3CH2NH2], and..
5.0ml of 12 M NH3 is added to 500ml of 0.050 M AgNO3. What concentration of silver ion will exist after equilibrium is established. {Kf for Ag(NH3)2 is 1.5 x 10^7
Explain Net Ionic Equations and Balancing, These are only eight out of a fifty-three question hand out, but with eight answers to reference off of I think I'll be far more successful in my attempts at this.
In the process, a photon of wavelength 1.28Ã-10-6 m is emitted. What was the value of the principal quantum number for the higher energy level?
Which of the following observations is the strongest argument that in favor of the hypothesis that protein structure and function are related?
Write balanced net ionic equation for the neutralization of equal molar amounts of HNO_2 and KOH
Find the pH of a solution after 0.10 mol of HCl is added to 1.0 L of a buffer solution that contains 1.40 M NH3 and 0.90 M NH4+.
An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?
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