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1) Estimate the magnitude of the absolute error and percent error in the measured sample volumes. Compare those errors to the errors that occur when measuring volumes of approximately 8 mL, as is normally done in this experiment. Assume that the graduated cylinder used to measure all of the volumes has 0.1 mL graduations.
2) Based on your answer to (1), would you be more or less confident about your density measurement if you used the smaller sample volume, rather than the normal 8 mL sample volume? Briefly explain.
What might happen to your calculated NaOH morality if you use tap water rather than deionizer (purified) water to dissolve the KHP crystals or to rinse down the walls of the flask during the titration
A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rises from 25.0°C to 62.3°C, determine the heat capacity of the calorimeter. The molar mass of ethanol is 46.07 g/mol.
Write the ionic equation and net ionic equation for the following reactions. Show all work for each balanced equation a. HCl(aq)+ NaOH(aq) b. CH3COOH (aq) + NaOH (aq)
How many miles could you drive for $3.90 if the gas mileage of your car is 14.0 km/liter of gasoline and the price of gasoline is $0.96/gal
how far away from equilibrium is the concentration of ADP and ATP in the cell? Answer A. equal B. slightly different C. greater than two orders of magnitude different D. greater than 6 orders of magnitude different E. greater than 12 orders of mag..
The charges of the ions in an ionic compound affect the strength of the electrostatic attraction holding that compound together. Based on ion charges, rank these ionic compounds by their expected melting points.
What is the molar mass of a compound if one mole of the compound contains two moles of oxygen atoms, 6.022 × 1024 hydrogen atoms, and 60.05 grams of carbon?
1. during the titration several milliliters of deionized water are added to the erlenmeyer flask containing the khp
isotope has a natural abundance of 57.21% and an atomic mass of 120.90382 amu. Calculate the percent abundance and atomic mass of the 123^Sb isoyope
If 20.0 ml of glacial acetic acid (pure ) is diluted to 1.20 L with water, what is the of the resulting solution. The density of glacial acetic acid is 1.05.
Acetylene gas (C2Hs) is produced as a result of the reaction CaC2(S)+2H2O(l)-> C2H2(g)+Ca(OH)2(aq).
a toothpaste contains 0.24 by mass sodium fluoride used to prevent dental caries and 0.30 by mass triclosan rm
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