Write the balanced NET ionic equation for the reaction when Na:S and NISO4 are mixed in aqueous solution. If no reaction occurs, write only NR.
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Q: net ionic equation
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A: A balanced chemical equation for the reaction of the white substance with water has to be given.
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- Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.Write a charge balance for a solution of H2SO4 in water if the H2SO4 ionizes to HSO4 and SO+4.Although sulphuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO42- ions, true or false? Justify your answer.
- Arsenic(III) oxide (As2O3) is available in pure form and is a useful (but carcinogenic) primary standard for oxidizing agents such as MnO4-. The As2O3 is dissolved in base and then titrated with MnO4- in acidic solution. A small amount of iodide (I - ) or iodate (IO3-) is used to catalyze the reaction between H3AsO3 and MnO4-. As2O3 + 4 OH - 2 HAsO32- + H2OHAsO32- + 2 H+ H3AsO35 H3AsO3 + 2 MnO4- + 6 H+ 5 H3AsO4 + 2 Mn2+ + 3 H2O (a) A 3.209 g aliquot of KMnO4 (FM 158.034) was dissolved in 1.000 L of water, heated to cause any reactions with impurities to occur, cooled and filtered. What is the theoretical molarity of this solution if no MnO4- was consumed by impurities? M(b) What mass of As2O3 (FM 197.84) would be just sufficient to react with 25.00 mL of the KMnO4 solution in part (a)? g(c) It was found that 0.146 8 g of As2O3 required 29.98 mL of KMnO4 solution for the faint color of unreacted MnO4- to appear. In a blank titration, 0.03 mL of MnO4- was required to produce enough…Write a charge balance for H2SO4 in water.The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………
- a 25.00 mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.00 mL aliquots of the diluted solution required an average of 34.88 mL of 0.09600 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid (MM:60g/mol). Consider the correct significant figures of your answer and do not forget the unit.The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.1) For an open system with PCO2=10−3.5 atm what fraction of the total carbonate is in the form of CO32− at pH 10.63? 2) Using paleolimnological methods it is possible to estimate past pH values of surface waters. If the estimate of pH is 5.787 , what is the corresponding PCO2? in atm.
- A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)
