Question

In: Chemistry

In an experiment, a student was asked to measure the desity of an unknown liquid. He...

In an experiment, a student was asked to measure the desity of an unknown liquid. He was given a small flask, which he found to have a mass of 32.6195 grams when empty. He filled the flask with water at 21.6 (0.997860 g/mL) degrees C and found the full flask to have a mass of 156.8995 grams. The student then emptied and dried the flask and then filled the flask with an unknown liquid. The mass of the flask filled with the unknown liquid was 134.2515 grams. Determine the volume of the flask and density of the unknown liquid.

Expert Solution

Answer – We are given, mass of empty flask = 32.6195 g ,

Mass of flask + water =156.8995 g , density of water = 0.997860 g/mL

Mass of flask + unknown liquid = 134.2515 g

Mass of water = Mass of flask + water – mass of empty flask

= 156.8995 g - 32.6195 g

= 124.2800 g

Density of water = mass of water / volume of water

So, volume of water = mass / density

= 124.2800 g / 0.997860 g.mL^-1

= 124.5465 mL

So, volume of water = volume of flask = 125.5465 mL

Mass of unknown liquid = 134.2515 g -32.6195 g

= 101.6320 g

So, density of unknown liquid = mass / volume

= 101.6320 g / 125.5465 mL

= 0.8160 g/mL

queen_honey_blossom answered 2 years ago

In an experiment, a student was given 2.0 g of an unknown salt either CoCl2 or...

In an experiment, a student was given 2.0 g of an unknown salt either CoCl2 or CoS-2H2O. During the experiment, the student isolated 0.93g of Co. Which salt did he start with? Why?

A student attempted to identify an unknown compound by the method described in this experiment. When...

A student attempted to identify an unknown compound by the method described in this experiment. When he heated a sample weighing 1.031 g the mass went down to 0.688 g. When the product was converted to a chloride the mass went up to 0.748 g. (Answers I got are in bold) 1.Explain if you believe the sample to be a carbonate or hydrogen carbonate. (I said it is a hydrogen carbonate due to the loss of mass) 2.Write the two...

1. A student attempts to identify an unknown compound by the method used in this experiment....

1. A student attempts to identify an unknown compound by the method used in this experiment. She finds that when she heated a sample weighing 0.5015 g the mass went down appreciably, to 0.3432 g. When the product was converted to a chloride, the mass went up, to 0.3726 g. a. Is the sample a carbonate? ____________ Give your reasoning. b. What are the two compounds that might be in the unknown? ____________ and ____________ c. Write the chemical equation...

In a student experiment, a constant-volume gas thermometer is calibrated in liquid nitrogen (−196°C) and in...

In a student experiment, a constant-volume gas thermometer is calibrated in liquid nitrogen (−196°C) and in boiling pentane (36.1°C). The separate pressures are 0.347 atm and 1.436 atm. Hint: Use the linear relationship P = A + BT, where A and B are constants. (a) What value of absolute zero does the calibration yield? °C (b) What pressure would be found at the freezing point of water? atm (c) What pressure would be found at the boiling point of water?...

Many techniques exist to measure the surface energy between a liquid and a liquid or a...

Many techniques exist to measure the surface energy between a liquid and a liquid or a liquid and a gas (see e.g. the wiki page). Methods to measure the surface energy between a solid and a fluid are rare, but still there is a method developed by Zisman (see e.g. here) that allows you to at least estimate it by extrapolation for solid/gas or solid/liquid, depending on the environment that you use in your experiment What I wonder: is there...

Please explain in detail. a) A student performed a calorimetry experiment. He combined 50.0 mL of...

Please explain in detail. a) A student performed a calorimetry experiment. He combined 50.0 mL of water at 85˚C and 50.0 mL of water at 22˚C in a coffee cup calorimeter. The final temperature of the water was 45˚C. What was the heat capacity of the calorimeter? b) The same calorimeter was used to find the specific heat of a metal. He heated 95.22 grams of the metal in a boiling water bath (99˚C). After adding this hot metal to...

A student does an experiment to determine the molar solubility of lead(II) bromide. He constructs a...

A student does an experiment to determine the molar solubility of lead(II) bromide. He constructs a voltaic cell at 298 K consisting of 0.821 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead bromide solution and a lead electrode in the anode compartment. If the cell potential is measured to be 5.60*10-2 V, what is the molar solubility of lead bromide at 298 K determined in this experiment? mol/L

One student set up the experiment to study the behavior of the pendulum, he did 6...

One student set up the experiment to study the behavior of the pendulum, he did 6 trials, keeping the amplitude in 15 degree and changing the length of the pendulum, with a timing device he determines the period for different lengths. The experimental data is shown below, trial L[m] T[s] 1 0.5 1.37 2 0.6 1.50 3 0.7 1.63 4 0.8 1.74 5 0.9 1.85 6 1 1.96 To examine more carefully how the period, T depends on the pendulum...

A student does an experiment to determine the molar solubility of lead(II) iodide. He constructs a...

A student does an experiment to determine the molar solubility of lead(II) iodide. He constructs a voltaic cell at 298 K consisting of 0.730 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead iodide solution and a lead electrode in the anode compartment. If the cell potential is measured to be 8.05×10-2 V, what is the value of Ksp for lead iodide at 298 K based on this experiment? Ksp for PbI2 =...

1. A psychology instructor asked each student to report the number of hours he or she...

1. A psychology instructor asked each student to report the number of hours he or she spent preparing for an exam. In addition, the instructor recorded the number of errors made on each student’s exam. The data are as follows: Hours (X) Errors (Y) 0 19 1 6 2 2 4 1 4 4 5 0 3 3 5 5 SSX =...