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1. The density of the solution is 0.982 g/mL and the density of water is 1.00
g/ml. If the solution is composed of 30.6 g NH3 in 81.3 g of H2O. Compute for;
a. mole fraction of NH3
b. molarity of NH3
c. molality of NH3
2. Given the reaction, H3PO4 + 3 NaOH Na3PO4 + 3 H2O, what is the
mass of 0.20 M H3PO4 needed to react with 100 ml. of 0.10 M NaOH?
1. Why does the Department of Health (DOH) recommends the use of 70% rubbing alcohol than 40% as a precautionary measure against corona virus?
2. Why does the Department of Environment and Natural Resources, (DENR) concern on the cauliform level, in parts per million, during the rehabilitation of beaches in Boracay? Research on the tolerable level of cauliform.
1. What is the percent by mass concentration of 41.0 g of sodium chloride
(NaCl) dissolved in 331 g of water (H2O)?
2. What is the percent by volume concentration of 25 ml ethanol (C2H5OH) in
75 ml solution?
3. What is the mass in grams of potassium nitrate (KNO3) needed to prepare
650 ml of 3.2 M KNO3 solution?
4. What is the molal concentration of a solution that contains 16 g of silver
nitrate (AgNO3) in 80 ml of water.
5. What is the molarity of 15.2 % by mass hydrogen peroxide (H2O2)? The
density of the solution is 1.01 g/ml.
Complete the balanced chemical equation for the reaction of CaCO3 and HCl
producing CaCl2, H2O and CO2. Fill in the concept map if we need to find the volume
of HCl given its molarity and mass of CaCO3.
Balanced Chemical Equation:
___ CaCO3 + ___ HCl ___ CaCl2 + ___ H20 + ___ CO2
Concept Map:
Mass of CaCO3,__________,___________,Volume of HCl
A 100 mL concentrated sulfuric acid (normally an Analytical Reagent, AR) will be weighed exactly to be used in a back-titration analysis. Explain how you will do this in the laboratory.
When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the limiting reagent and mass of PbSO4 when a 1.25 L solution of 0.0500 M Pb(NO3)2 and a 2.00 L solution of 0.0250 M Na2SO4 are mixed. (Hint: start first by balancing the equation of the reaction between Na2SO4 and Pb(NO3)2
Beaker
1
2
3
4
5
6
Sample Volume (mL)
1000
1000
1000
1000
1000
1000
Coagulant
(ppm)
12
14
16
18
20
22
SG of Coagulant: 1.22
Calculate what is the dosage in ml for 12ppm, 14ppm, 16ppm, 18ppm, 20ppm, 22ppm in the attached table for Jar Test purpose?
What volume (in L) of 0.246 M HNO3 solution is required to react completely with 38.6 mL of 0.0515 M Ba(OH)2?Ba(OH)2 + 2HNO3 → Ba(NO3)2 + 2H2O
Illustrate the phase diagram of a substance given with the following points: a triple point at 0.70 atm and 80 ºC; a normal freezing point at 100 ºC; a normal boiling point at 350 ºC; and a critical point at 1.6 atm and 810 ºC. For this,
complete the following:
1. Roughly sketch the phase diagram, using units of atmosphere and degree
Celsius. Label the area 1, 2, and 3, and points T and C on the diagram.
2. Describe what one would see at pressures and temperatures above 1.25 atm and 300 ºC.
3. Describe the phase changes from 100 ºC to 200 ºC at 1.5 atm.
4. What exists in a system that is at 1 atm and 100 ºC?
5. What exists in a system that is at 1 atm and 325 ºC?
What is the molarity of 0.650L of solution containing 63g of Nacl
