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Write is the phase labels for the molecular equation and find the balanced net ionic equation.
Ca(C2H3O2)2 + H2C2O4 -> CaC2O4 + 2HC2H3O2
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- 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.Write the balanced NET ionic equation for the reaction when aqueous SrBr₂ and aqueous K₂SO₄ are mixed in solution to form solid SrSO₄ and aqueous KBr. Be sure to include the proper phases for all species within the reaction.Do you agree/disagree with the following statement below? State your reasons. "Classical precipitation gravimetric analysis is best used towards the end of quantitative analysis while classical volumetric analysis is best used as the first technique to quantify analytes."
- Write the balanced COMPLETE ionic equation for the reaction when aqueous MgSO₄ and aqueous Ba(NO₃)₂ are mixed in solution to form aqueous Mg(NO₃)₂ and solid BaSO₄. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. ☐⁴⁻ ☐³⁻ ☐²⁻ ☐⁻ ☐⁺ ☐²⁺ ☐³⁺ ☐⁴⁺ 1 2 3 4 5 6 7 8 9 0 ☐₁ ☐₂ ☐₃ ☐₄ ☐₅ ☐₆ ☐₇ ☐₈ ☐₉ ☐₀ + ( ) → ⇌ (s) (l) (g) (aq) Ba Mg S O N ResetWrite the balanced dissociation equation for solid mercury(I) acetate in aqueous solution. If it does not dissociate, simply write only NR. Be sure to include the proper phases for all species within the reaction.Prepare 0.1 M solutions of NaOH and 0.1 M ethyl acetate using high-purity distilled water. So, weight desired amount of NaOH and ethyl acetate and dissolved in dH2O to prepare stock solution in equal molarity. Mw (NaOH) = 40.0 g/mol , Mw (EtOAc)= 88.1 g/mol, Density(EtOAc): 0.898 g/cm3
- Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. From the stock solution (0.020 M), pipet 4.00 mL and dilute to 100.00 mL. From the diluted solution, pipet 0.00, 1.00, 1.50, 2.00, 2.50, 5.00 and 7.50 mL aliquots into 100 mL volumetric flasks. Dilute to mark. Determine the concentration of each standard solution and tabulate.Estimate the aqueous gram-solubility in g/L of mercury(I) chloride: Hg2Cl2(s) ↔ 2Hg+ (aq) + 2Cl– (aq), Ksp = 1.43×10–18 The molar mass of Hg2Cl2 is 472.06 g/mol.What volume of a 0.186 molL−1 Na3PO4 solution is necessary to completely react with 91.9 mL of 0.103 molL−1 CuCl2?v
- Consider the reaction of Potassium Phosphate and Nickel (II) Bromide, where 15.00 ml of 0.7000M K3PO4 is mixed with 15.00ml of 0.2000M NiBr2 (and the final volume is 30.00 ml, that is there is no change in volume upon mixing). Your answer has to include all of the following: What is the limiting reagent? What is the identity and mass of precipitate formed? What is the concentration of the alkali metal that is a spectator ion? What is the concentration of the excess phosphate?For a given solution containing an ionic compound, what is the relationship between Q, Ksp and the relative saturation of the solution ?During the precipitation of lead sulfate with sulfuric acid, if bismuthyl sulfate is also formed because of the addition of too much water, describe a method of separating them, then illustrate with a balanced ionic equation