2. A student was given five known solutions and asked to study their interactions. Thesolutions were 0.1 M Na SO, 0.1 M NaCl, 0.1 M Ba(NO₂), 0.5 M HCl, and 0.3 M Na₂CO₂-a. To determine the behavior of these solutions, the student mixed them systemically in pairsand used the grid below to record the observations. Based on your lab data andobservations, fill in the grid, indicating what observations the student would have madewhen each pair of solutions was mixed. Use "N.R." to indicate no reaction, "ppt" forprecipitate (or solid) formed, and "gas" for a released gas.NaClsolutionsBa(NO₂laNa 50₁Na CO₂HCINaClsolutionsTest Tube Bb. The student was then given the same set of five solutions, but this time in test tubes labeledA, B, C, D, and E. When these solutions were mixed, the student recorded the followingobservations.Test Tube CEDCBAAN.R.N.R.HCIN. R.muN.R.white ppt. N.R.N.R.Na₂CO₂сwhite pptN.R.Na₂SO Ba(NO₂)Using the information from part 2a, identify the solution in each test tube.Test Tube ATest Tube DTest Tube EDgasE12

1) Solutions of Ba(NO3)2 and NaCl: NR Reaction: Ba(NO3)2(aq) + 2NaCl(aq) = BaCl2(aq) +…

2. A student was given five known solutions and asked to study their interactions. The solutions were 0.1 M Na SO, 0.1 M NaCl, 0.1 M Ba(NO), 0.5 M HCl, and 0.3 M Na₂CO₂. a. To determine the behavior of these solutions, the student mixed them systemically in pairs and used the grid below to record the observations. Based on your lab data and observations, fill in the grid, indicating what observations the student would have made when each pair of solutions was mixed. Use "N.R." to indicate no reaction, "ppt" for precipitate (or sollid) formed, and "gas" for a released gas. solutions NaCl HCI Na CO Ba(NO₂) Na 50₁ NaCO HCI Naci solutions E D C b. The student was then given the same set of five solutions, but this time in test tubes labeled A, B, C, D, and E. When these solutions were mixed, the student recorded the following observations. A A N.R. N.R. white ppt. N. R. N.R. N.R. N.R. Na 50 с white ppt. N.R. D gas Ba(NO₂) Using the information from part 2a, identify the solution in each test tube. Test Tube A Test Tube D Test Tube B Test Tube E Test Tube C E

2. A student was given five known solutions and asked to study their interactions. The solutions were 0.1 M Na SO, 0.1 M NaCl, 0.1 M Ba(NO), 0.5 M HCl, and 0.3 M Na₂CO₂. a. To determine the behavior of these solutions, the student mixed them systemically in pairs and used the grid below to record the observations. Based on your lab data and observations, fill in the grid, indicating what observations the student would have made when each pair of solutions was mixed. Use "N.R." to indicate no reaction, "ppt" for precipitate (or sollid) formed, and "gas" for a released gas. solutions NaCl HCI Na CO Ba(NO₂) Na 50₁ NaCO HCI Naci solutions E D C b. The student was then given the same set of five solutions, but this time in test tubes labeled A, B, C, D, and E. When these solutions were mixed, the student recorded the following observations. A A N.R. N.R. white ppt. N. R. N.R. N.R. N.R. Na 50 с white ppt. N.R. D gas Ba(NO₂) Using the information from part 2a, identify the solution in each test tube. Test Tube A Test Tube D Test Tube B Test Tube E Test Tube C E

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 94AP

See similar textbooks

Similar questions

1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.219 M CsOH. Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction.
As part of the analysis of water samples, the hardness of water is commonly measured and calculated. It is commonly expressed in ppm by mass (parts per million) of CaCO3. Parts per million is also equivalent to milligrams of CACO3 per liter of water. In a sample taken by an environmentalist, he was able to observe a hardness count of 205 mg CacO3/L. Given this hardness count of the sample, what is the molar concentration of Ca2+ ions in the water sample?
The solubility of Ca(OH)2 is measured and found to be 0.912 g/L. Use this information to calculate a Ksp value for calcium hydroxide.
The solubility of an ionic solid in water is quantified by this expression: Ksp Kc Keq Ka or Kb
Calculate the solubility and molar solubility of Cu3(PO4)2 (MW=380.58 ; Ksp=1.4x10-37).
The solubility of aqueous PbCr2O7 at 25 oC is 1.55 x 10–2 g/L at 25.0 oC. Calculate the Ksp of PbCr2O7 at this temperature. MM PbCr2O7 = 423.188 g/mol
Consult a reference such as the “CRC Handbook of Chemistry and Physics” and look up the solubility of lead(II) chloride in both hot water and cold water. _________? g/L (0 °C) _________? g/L (20 °C) _________? g/L (100 °C) Based on these data, why is the use of hot water critical to the success of this experiment?
Assume that the solubility of carbon dioxide gas in pop at 5oC is 0.586 g/100 mL and at 20oC its solubility is 0.169 g/100 mL. What mass of carbon dioxide gas will escape from a 355-mL can of Coke that has been taken out of the fridge and has been sitting open at 20oC?
The solubility of CO2 in water is a function of pressure.Calculate the concentration of CO2 in water when ???2 = 2.5 × 10−4 bar
Derive an effective Henry’s constant formula for ammonia (NH3) dissolved in water
The addition of a small amount of a salt, such as (NH4)2SO4, to a solution containing a charged protein increases the solubility of the protein in water. This observation is called the salting-in effect. However, the addition of large amounts of salt can decrease the solubility of the protein to such an extent that the protein precipitates from solution. This observation is called the salting-out effect and is used widely by biochemists to isolate and purify proteins. Consider the equilibrium PXν(s) ⇋ Pν+(aq) + ν X−(aq), where Pν+ is a polycationic protein of charge ν+ and X− is its counterion. Use Le Chatelier’s principle and the physical principles behind the Debye–Hückel theory to provide a molecular interpretation for the salting-in and salting-out effects.