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Q: Calculate the normality of 0.2M Na2CO3 (M.wt = 106).
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Calculate the normality of 5.627 g/L K₂Cr₂O₇ (294.19) in the reaction: Cr₂O₇²⁻ + 14H⁺ + 6e⁻ ⟶ 2Cr³⁺ + 7H₂O *
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- In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:The Kc for the reaction 2A (aq) ⇌ 3 B (aq) is 0.085. What is Kc for the reaction 3 B (aq) ⇌ 2A (aq)?Twenty grams of potassium dichromote (K2C2O7) is dissolved in 150 mL of water. What is its normality as a solution? a) 0.70N b) 1.81 N c) 1.41 N d) 0.91 N The solution in the previous problem was used in titration producing chromium(II) oxide (CrO). What is the normality of the solution in the said reactin? a) 0.70N b) 1.81 N c) 1.41 N d) 0.91 N
- Calculate the normality of 0.2M Na2CO3 (M.wt = 106).A solution of permanganate contains 2.608 grams of KMnO4 per 750 mL. What is the normality of the solution and what is the value of 1.000 mL in terms of H2O2?8. 39.24 mL of permanganate solution reacts with 0.241 g sodium oxalate according to the following reaction. Determine the normality for this permanganate solution. Na2C2O4 + KMnO4 + H2SO4 --> MnSO4 + CO2 + Na2SO4 + K2SO4 + H2O detirmine equivalent weight for sodium oxalate detirmine equivalents of sodium oxalate
- 1. Calculate the normality of 0.321 g sodium carbonate (106.0 g/mol) when it is mixed in a 250 mL solution. 2. What is the normality of 0.0521 M H3PO4? 3. A12.5-mL portion of a base solution of an element from group 2A is diluted to 500 mL; the resulting concentration of this solution is determined to be 0.125 M. What is the normality of the original solution. 4. A sample of USP-grade citric acid (H3C6H5O7, three titratable protons) is analyzed by titrating with 0.1087 M NaOH. A 0.2678-g sample requires 38.31 mL of the titrant for titration. A. What is the normality of the titrant? B. What is the stoichiometric relationship between the analyte and the titrant? C. How many moles of the titrant were consumed to react with the analyte? NOTE: please include the given, the unknown, the chemical reaction, the calculation process, and the final answer with the proper number of significant figures.1. Calculate the equivalent weight of KMnO₄ in the following reaction: MnO₄⁻ + CN⁻ + H₂O ⟶ MnO₂ (s) + CNO⁻ + OH⁻) 2. Calculate the normality and molarity of a 15.0% (by weight) H₂SO₄ solution with a specific gravity of 1.090. * 3. To what volume should 100 mL of the above solution be diluted to prepare 1.50 N solution?A student uses 7.500 grams of oxalic acid (H₂C₂O₄) to make 250.0 cm³ of solution in a volumetric flask. She then transfers 20.0 cm³ of the solution to a conical flask with a pipette. What is the concentration in mol·dm⁻³ of the oxalic in the conical flask?
- Calculate the normality of 12.5 g of potassium permanganate (KMnO4) in 475 mL solutionIdentify and explain the mistakes made in the following laboratory protocols: A 10.00 mM solution of glucose (FW 180.16 g/mole) was prepared by first adding 180.16 mg of glucose to a 100 mL empty volumetric flask, and then DI H2O was added to the volumetric flask until the meniscus reached the 100 mL volume mark. The flask was capped and the solution vigorously mixed until the glucose completely dissolved.A flask of 25.0 mL with an unknown concentration of magnesium hydroxide completely reacts with 18.0 mL of 1.0 M hydrochloric acid solution according to the equation : HCl (aq) + Mg(OH)2 (aq) -> MgCl2(aq) + H2O (l) Determine the concentration of the magnesium hydroxide solution using dimensional analysis when possible.
