Write a net ionic equation for the overall reaction that occurs when aqueous solutions of sodium hydroxide and sulfurous acid (H2SO3) are combined.
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Write a net ionic equation for the overall reaction that occurs when aqueous solutions of sodium hydroxide and sulfurous acid (H2SO3) are combined.
Assume excess base. Use the pull-down boxes to specify states such as (aq) or (s).
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- Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. CH3OH(aq) =?Given the mole ratio of HCl to NaOH is 1:1 in the balanced acid base reaction A 15.52mL sample of HCl is titrated to endpoint witg a 32.08mL sample of NaOH, which has a known molarity of 0.976M. How many moles of NaOH were used in this reaction?
- Write the balanced NET ionic equation for the reaction when ZnCl₂ and KOH are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.If weak acids ionize only a few percent in aqueous solution, why is it possible to fully neutralize a weak acid by reacting it with the stoichiometric equivalent of sodium hydroxide solution, NaOH(aq)?Consider these compounds: A. Al(OH)3 B. Ag3PO4 C. Zn3(PO4)2 D. Ca3(PO4)2 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that barium phosphate is more soluble than , and barium phosphate is less soluble than . It is not possible to determine whether barium phosphate is more or less soluble than by simply comparing Ksp values.
- Oxalic acid dihydrate (H2C2O4 • 2H2O, molecular weight = 126.07 g/mol), a diprotic acid, can also be used to standardize NaOH solution. If 0.284 g of H2C2O4 • 2H2O is dissolved in water and titrated to the equivalence point with 16.37 mL of NaOH, what is the molarity of the NaOH solution?Complete the equation for the reaction of NaHCO3(s) with HC2H3O2(aq). Include phase symbols.Write the balanced NET ionic equation for the reaction when NH₄Br and Pb(NO₃)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
- A 10.0 mL sample of household ammonia solution required 25.10 mL of 0.245 M HNO3 for neutralization. Calculate (a) the molar concentration of the ammonia and (b) the mass/mass % concentration of ammonia(17.04 d/mol), given a solution density of 0.985 f/mL. HNO3(aq) +NH3(aq) ---> NH4NO3(aq)Iodometry is a standard method for redox titration. In many indirect methods one lets the analyte (the substance whose concentration is to be determined) react with iodide ions as then forms triiodide ions, I3- . The amount of triiodide ions is then determined by titration with thiosulphate ions, S2O32- which then form tetrathionate ions, S4O62- whereby the triiodide ions change into iodide ions. Determine the mass of triiodide ions in a solution from the following data. The sample containing triiodide ions was titrated with a 0.01002 M sodium thiosulfate solution of which 18.38 mL were required.Complete and balance each of the following equations for acid-base reactions. H2SO4(aq)+Ca(OH)2(aq)→H2SO4(aq)+Ca(OH)2(aq)→ Express your answer as a chemical equation. Identify all of the phases in your answer.