6ASAP Compounds containingthese ions are SolubleNO3-Na+, K+, NH4+CF, Br, ISO4²-Compounds containingthese ions are InsolubleS², CO², PO4³OHExcept for thoseContainingNoneNoneAgt. Hg2+, Pb2+Ba²¹, Pb²¹, Ca²¹Except for thoseContainingNa+, K+, NH4+Na+, K+, Ba2+, Ca²+7. Write the balanced molecular, complete ionic and net ionicequations for this exchange (double-displacement) reaction.Cal₂ (aq) + Na3PO4 (aq)-

Given reaction: CaI2 (aq) + Na3PO4 (aq) → We have to write the balanced molecular, complete ionic,…

Compounds containing these ions are Soluble NO₂™ Na, K, NH₂ CF, Br, I SO4² Compounds containing these ions are Insoluble S², CO², PO4³ OH Except for those Containing None None Ag, Hg2+, Pb2+ Ba², Pb²¹, Ca Except for those Containing Na, K, NH4+ Na+, K+, Ba²+, Ca²+ 7. Write the balanced molecular, complete ionic and net ionic equations for this exchange (double-displacement) reaction. Cal₂ (aq) + Na3PO4 (aq)-

Compounds containing these ions are Soluble NO₂™ Na, K, NH₂ CF, Br, I SO4² Compounds containing these ions are Insoluble S², CO², PO4³ OH Except for those Containing None None Ag, Hg2+, Pb2+ Ba², Pb²¹, Ca Except for those Containing Na, K, NH4+ Na+, K+, Ba²+, Ca²+ 7. Write the balanced molecular, complete ionic and net ionic equations for this exchange (double-displacement) reaction. Cal₂ (aq) + Na3PO4 (aq)-

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.12QAP

See similar textbooks

Similar questions

You are supplied with the following: / Jy word voorsien van die volgende: NaCl(Mr= 58,443 g /mol) 2.5MTris-Cl, pH 8 solution /oplossing (1 Litre) EDTA,natriumsout(Mr= 380,2g/mol) 10% sodium dodecyl sulphate solution / natriumdodecyl sulfaat oplossing Proteïnase K solution / oplossing (50 mg dissolved / opgelos in 1 ml ddH2O) You need a digestion buffer consisting of the following: / Jy moet 'n verteringsbuffer op maak wat uit die volgende bestaan: 15m M NaCl 75 mM Tris-Cl,pH 8 16 mM EDTA,pH 8 0.8% sodium sulphate / natrium dodecyl sulfaat 0,75 mg/ml proteïnase K How will you prepare 500 ml of the digestion buffer? Show all your steps and calculations. Remember to explain exactly how you will make it up.
One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?
Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.
Given the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions shown below: [1] Fe(OH)3 3 H+ à Fe3+ + 3 H2O Ksp = 8.4 x 10^4 ∆ Gr0 = -28 KJ/mol Solubility of Fe(OH3) = 7.468 [2] FeOOH + 3 H+ à Fe3+ + 2 H2O Ksp = 8.8 x 10^-2 ∆ Gr0 = 6 KJ/mol Solubility of FeOOH = 0.353 QUESTION: [A] How much Fe3+ from ferrihydrite would dissolve at pH 2 ? [B] How much Fe3+ from ferrihydrite would dissolve at pH 7 ? [C] How much Fe3+ from goethite would dissolve at pH 2 ? [D] How much Fe3+ from goethite would dissolve at pH 7 ?
When 0.650g of compound W is dissolved in 27.8g biphenyl (Kf= 8.0oC/ molal, fp= 70.0oC), the fp of the solution is 68.44oC. What is the MW of W?
Give solution of the all three subparts in clear handwritten!
Estimate the fraction, f, of F6P in a solution in which G6P and F6P are in equilibrium at 25 °C given that ΔrGΘ = +1.7 kJ mo l-1 at that temperature, which implies that K=0.50.
One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.
The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?