A student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ(NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate forms yes red purple calcium acetate lithium acetate No precipitate forms lithium hydroxide lithium permanganate none none colourless White precipitate yes red colourless forms No precipitate yes red colourless forms yellow- No precipitate yes colourless red forms

A student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ(NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate forms yes red purple calcium acetate lithium acetate No precipitate forms lithium hydroxide lithium permanganate none none colourless White precipitate yes red colourless forms No precipitate yes red colourless forms yellow- No precipitate yes colourless red forms

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The researcher extracts a sample of well water and prepares it for TXRF analysis with a 10.00 mg/L V internal standard, like the calibration standards. The result produces SCa = 69297.81 and SV = 13481.2.Determine the concentration of Ca.
KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
In the laboratory, a student was tasked to prepare a stock solution of HCl for titration. The available analytical grade HCl solution in the stock room was labelled 35% w/v HCl. The student proceeded to prepare the stock solution by mixing 10mL of the HCl solution with 490mL of analytical grade water. Then, the solution was further diluted by adding 5mL, since the total volume of the solution did not reach the 500mL etched mark on the volumetric flask. To prepare the titrant, the student mixed 10mL of the stock solution, then added 40mL of analytical grade water. The titrant was subsequently used to determine the concentration of two titrand. *Use the table as a reference 1. What is the normality of the available HCl reagent in the stock room?* 5.08 N 10.15 N 20.3 N 11.0 N None of the choices 2. What is the normality of the stock solution of HCl?* 0.09N 0.10N 0.11N 0.12N None of the choices 3. What is the normality of the titrant?*…
A 0.512 g sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter. The residue was taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH4PO4.6H2O by addition of Mg2+ followed by aqueous NH3. After being filtered and washed the precipitate was converted to Mg2P2O7 by ignition at 1000 0C and the residue weighed 0.1151g. (a) What is the Gravimetric Factor to convert Mg2P2O7 to P? (b) Calculate the percent P in the sample could you type it out please
A K2SO4 solution is prepared by weighing out a certain amount of the pure solid reagent,dissolving it to 500.0 mL in a volumetric flask. An aliquot was taken from this solution.of 25.00 ml and diluted to 500.0 ml. An aliquot of 5.00 was taken from this new solution anddiluted to 50.00 ml. A chemical analysis of this new solution showed a 0.100%(w/v)in K+. Calculate the weight of the pure solid K2SO4 used for the preparation of the original solution.and its concentration in each volumetric flask. The answer is 2.23x10^2g
Magnesium Chloride is available as magnesium chloride hexahydrate in an injectable solution that supplies 1.97 mEq of magnesium per milliliter. What is the percent strength of magnesium chloride hexahydrate in this solution?
Calculate ΔG'° for a reaction proceeding under biochemical standard conditions with a K'eq of 2.32. Give your answer in units of kJ/mol, but do not include the units as part of your answer (give the number only)
Give specific examples of these chemical incompatibilities and their remedies 1. Precipitation,oxidation, redox reactions hydrolysis, racemisation, efffervescence, colour change,incompatibity with containers, and formulation of insoluble complexes and polymerisation
An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.
Calculate (delta)G (naught) for the process. Standard State: 1 M
Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. The equilibrium expression for the process is: Na2B4O5(OH)4 10H2O (s) ⇌ 2 Na+ (aq) + B4O5(OH)4 2- (aq) + 10H2O(l) Since liquid water and solid borax are not included in the Ksp expression, the solubility product expression associated with this reaction is: Ksp = [Na+]2[borate] The concentration of the borate ion in equilibrium with solid borax can be determined by titration with HCl based on the following equation: B4O5(OH)42- + 2HCl(aq) + 3H2O (l) → 4 H3BO3(aq)+2Cl-(aq) The Ksp for borax will be evaluated at room temperature at 5oC. Knowing the Ksp values at two temperatures allows the use of the following equations to calculate the change in enthalpy and Gibbs free energy: In(Ksp1/Ksp2)=ΔH/R((1/T2)-(1/T1)) ΔGo= - RT InKsp Once ΔHo and ΔGo are known, you can find…
Calculate the Free Gibb’s energy, kJ/mol, for a saturated solution of CdCO3 at 25.0°C. Ksp = 5.2 x 10-12