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The neutralization of 50.0 mL of 1.00 M hydrochloric acid with 50.0 mL of 1.00 M sodium hydroxide causes a 6.7°C increase in temperature. Predict how the following changes to the experimental protocol would affect the value of the change in temperature.
The temperature change depends on the moles of water produced (moles of reaction) and the mass of the solution. Assume that the density of each solution is 1.0 g/mL.
a. using 100.0 mL of 1.00 M hydrochloric acid and 100.0 mL of 1.00 M sodium hydroxide
b. using 50.0 mL of 2.00 M hydrochloric acid and 50.0 mL of 2.00 M sodium hydroxide
c. using 25.0 mL of 1.00 M hydrochloric acid and 75.0 mL of 1.00 M sodium hydroxide
d. using 25.0 mL of 1.00 M sulfuric acid and 75.0 mL of 1.00 M sodium hydroxide
Calculate the molarity of a Ca(OH)2 solution if it takes 25.0 mL to titrate 0.650 g of KHP in a standardization titration. (KHP has one H+ and a formula weight of 204.2 g/mol.)
8 ml of the HCl was used to titrate the pK_a 3.8 group; so 2 ml was enough to titrate the rest of the high pK_a group. The upper pK_a group must have begun the experiment as 80% acid form, 20% base form.
160 mL that contains 400 mg of NH3 and 980 mg of NH4NO3. (Given: Kb (NH3) = 1.8 x 10-5
Assume every breath a person took is 0.5L of air, figure out how many grams of Oxygen you consume at every breath. Now assume that you breathe 30 times per second, figure out how long it took for you to consume all the oxygen in a sealed room of 1..
determine at what pressure will pure H 2 O start to boil if its temperature is seventy five degree Celsius
2.914 gram sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temperature greater than 170 degrees celcius in a crucible until a constant mass is reached.
Explain why Lewis dot structure for S2Cl2 IS Cl - S - S - Cl why does the two sulfurs have to be beside each other and the two chlorines have to be the first and last?
Calculate the molarity of the solution. How many grams of KNO3 are needed to make 450 mL of a solution that is to contain 5.50 mg/mL of potassium ion?
gas evolution frequency is observed during the seperatory funnel extractions in this experiment. What is the identity of this gas and how is it formed?
Calculate the pH of the titration mixture after 10.0, 20.0 and 30.0 mL of base have been added. (the ka for acetic acid is 1.76 x 10^-5).
A 515 g piece of copper tubing is heated to 95.0°C and placed in an insulated vessel containing 57.0 g of water at 30.0°C.
Table salt (NaCl) and sugar (C12H22O11) are accidentally mixed A 5.00g sample is burned and 2.20-g of CO2 are produced. What is the mass percentage of the table salt in the mixture.
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