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Molarity of Na2S2O3 (stock solution). 0.100 M
Volume of diluted bleach titrated (taken from the volumetric flask). 10ml
Initial Burette Reading. 14.80
Final Burette Reading 25.60
Volume of Na2S2O3 used in the titration (mL). 10.80
Moles of Na2S2O3 used in the titration. 1.71
Moles of S2O3–2 used. 1.66
Moles of I2 initially present in titration mixture 0.83
Moles of NaOCl in the diluted bleach titrated. 0.415
Volume of bleach titrated. 1ml
Mass of NaOCl in commercial bleach titrated. ?
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 669669 mg of AgCl(s) in 100.0 mL of solution. The KspKsp of AgCl is 1.77×10−101.77×10−10.POTASSIUM PERMANGANATE AND SULFURIC ACID Place 10 drops of 0.1M potassium permanganate solution in a test tube. Add 2 drops of 6M sulfuric acid. Add drop by drop 0.1M sodium bisulfite solution until a definite color change is observed. Observations: Balanced chemical equation: H2SO4(aq) + 4KMnO4(aq) + 10NaHSO3(aq) → 6H2O(l) + 2K2SO4(aq) + 4MnSO4(aq) + 5Na2SO4(aq) What substance is responsible for the color change?
- Standardisation of the Permanganate Solution 5 C2O42-(aq) + 2 MnO4-(aq) + 16 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O Calculate the number of moles Na2C2O4 used in each of the three samples. Calculate the concentration of potassium permanganate in the standard solution for each of the three titrations you performed. Average the titration results and determine the concentration of Permanganate in the Standard Solution Recorded mass of sodium oxalate (Na2C2O4) in grams (g): Sample Mass M1 0.1134 M2 0.1136 M3 0.1124 M4 0.1100 Recorded initial- and final volume of Potassium Permanganate after titration: Sample Initial Volume in mL (Vi) Final Volume in mL (Vf) Total volume of KMnO4 used in mL. (Vf – Vi) 1 6.5mL 23.7mL 17.2mL 2 23.7mL 40.5mL 16.8mL 3 17.7mL 34.8mL 17.1mL 4 3.0mL 19.4mL 16.4mLDoes a precipitate form when a solution of calcium chloride and a solution of mercury(1) nitrate are mixed together? Choose one: O Yes, a precipitate is formed. O No, a precipitate is not formed.Calculate pCu in a 0.10 M CuSO4(aq) solution that is also 6.0 M in NH3. Cu²+ (aq) + 4 NH3(aq) [Cu(NH3)4]²+ (aq) Kf = 1.1 x 1013
- Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+H2O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration. A. How many moles of base were required to react completely with the acid in this reaction? _____mol Ca(OH)2 B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HClA student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 4 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.235, and Beer's law equation (the trend line from best fitting) as Abs = 243 x Concentration of FeSCN2+ + 0.012 Determine the equilibrium concentration for FeSCN2+ in mol/L.ab Consider the following reaction: Y s lock Enter the complete ionic equation for this reaction. Express your answer as a complete ionic equation. Identify all of the phases in your answer. 2H+ (aq) + 2Br (aq) + Ca²+ (aq) + 2OH- (aq) →2H₂O (1) + Ca2+ (aq) + 2Br (aq) esc Submit Previous Answers Answer Requested The complete ionic equation depicts the formation of ions in solution. The coefficients and subscripts of the balanced molecular equation are used to determine the coefficients of the complete ionic equation. Part B Enter the net ionic equation for this reaction. Express your answer as a net ionic equation. Identify all of the phases in your answer. Submit A chemical reaction does not occur for this question. *Mother to Son &....pdf A OD ES ΑΣΦ ! 1 Request Answer độc FI Q A N @ 2 F2 W S #3 X I control option command ? дв 80 F3 E D $ 4 C F4 R 2HBr(aq) + Ca(OH)2 (aq) → 2H₂O(1) + CaBr₂(aq) F % 5 V I FS T G 6 MacBook Air F6 B Y & 7 H 4 F7 U N * 8 J DII 1 M ( 9 K DD F9 O < 1 H ) 0 L…
- Complete the balanced molecular reaction for the following weak acid with a strong base. Be sure to include the proper phases for all species within the reaction. 1 + 2 Ca HNO₂(aq) + Ca(OH)₂ (aq) 3 H ²- 4 -> OH 5 = 6 H3O+ 6 (s) 7 H₂O 3+ 8 4+ N 9 0 (1) (g) (aq) O o5. Balance the following reaction. HCl(aq) + KMn04 (aq) +H2O2 (aq)MnClz (aq) +02 () +KCI (aq) + H20 (1) in an acid solutio a. When a reaction is said to be in an acid solution, what species are most commonly present?Cu(s) + 2 AgNO3(aq) ⇋ Cu(NO3)2(aq) + 2 Ag (s) If a mixture of excess Cu (s), 0.394 M AgNO3 (aq), and 0.136 M Cu(NO3)2 (aq) is placed in a reaction flask, calculate the equilibrium concentration (M) of AgNO3 (aq). Kc=2.174