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A) Explain how do you make 200mL of a 0.1 M solution of a substance that has a molecular weight of 121.1 g/mol?
B) If you take 10mL of the solution you made in A add 90 mL of water, mix and then take 5mL of the mixture and bring it to 25 mL, Explain what will be the concentration of the final solution in molars, millimolars and micromolars?
If a system has 2.00 x 10^2 kcal of work done to it, and releases 5.00 x 10^2 kJ of heat into its surroundings, what is the change in internal energy of the system
an ice bag containing 324 of ice at 0deg c was used to treat sore muscles. when the bag was removed the ice had melted
a certain protein was found to contain 0.639% zinc by mass. Determine the minimum molecular mass of the protein.
When dissolved in your stomach (pH=1) the concentration of aspirin (acetylsalicylic acid Ka = 3.0 x 10 ^-4) is 0.2 M. Calculate the % ionization of the aspirin.
the Grignard reagent containing more carbon atoms with the carbonyl compound containing less carbon atoms and scheme two involves the reaction of the Grignard reagent containing less carbon atoms with the carbonyl compound containing more carbon a..
A 0.150- M solution of chloroacetic acid (HC2H2ClO2) has a pH of 1.86. What is the value of Ka for this acid and the percent ionization?
The sulfide content in a pulp plant effluent is determined with a sulfide ion-slective electrode using the method of standard additions for calibration.
Explain why Copper metal does not dissolve in a typical strong acid such as hydrocholoric acid but will dissolve in 1M nitric acid
State the balanced formula equation complete ionic equation, and net ionic equation. If no precipitate forms state "No reaction".
sodium hydrogen carbonate and sodium chloride are both soluble in water. will a double replacement reaction take place
Define the enthalpy of FeBr3 (s) is -269 kj/mol and the enthalpy of the reaction 2Fe(s) +3Br2(g) ->2FeBr3 (s) is -631 kj/mol. Compute the enthalpy of evaporation of Br2 (l) which is liquid at 25C.
Iron metal is formed during the reduction of iron(III) oxide: Fe2O3 + 3CO 2Fe + 3CO2. When 28.4 kg of Fe2O3 react with 17.0 kg of CO and 4.2 kg of Fe are recovered, what is the percent yield for the reaction
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