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What is the net ionic equation for the following reaction? NazCO3(aq) + FeCI2(aq) --> FeCO3(s) + 2NaCl(aq)
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- A phosphate buffer contains KH2PO4 and K2HPO4. What is the net ionic equation for the buffering reaction that occurs when some HCl is added to the buffer solution? (A) H2PO4–(aq) + Cl–(aq) --> HPO42–(aq) + HCl(aq); (B) H2PO4–(aq) + H3O+(aq) --> H3PO4(aq) + H2O(aq); (C) HPO42–(aq) + Cl–(aq) --> PO43–(aq) + HCl(aq); (D) HPO42–(aq) + H3O+(aq) --> H2PO4–(aq) + H2O(aq);Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5143 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel the CO2: CaCO3(s) + 2H+ ⟶⟶ Ca2+ + CO2↑↑ + H2O The excess acid requied 39.96 mL of 0.1004 M NaOH for complete titration: OH- + H+ ⟶⟶ H2O Find the weight percent of calcite in the limestone.You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 17.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?
- 43. A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 125.0 mL Concentration of CH3COOH(aq): 1.263 M Volume of CH3COONa(aq): 106.0 mL Concentration of CH3COONa(aq): 1.279 M Determine the volume of 6.00 M HCl required to change the pH of this buffer by one pH unit. 18.15 mL 36.30 mL 21.87 mL 19.30 mL 43.73 mL42. A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 139.0 mL Concentration of CH3COOH(aq): 1.103 M Volume of CH3COONa(aq): 127.0 mL Concentration of CH3COONa(aq): 1.259 M Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base. 4.38 5.90 4.69 4.81 5.12What is the equilibrium expression for the following reaction? Zn(s) + 2NAOH(aq) + 2H2O(e) = NazZn(OH)4(aq) + H2(g)
- A 0.9600 M NaOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was titrated against an unknown acid. The volumes of NaOH(aq) titrated are shown in the table below. Volumes of NaOH(aq): Rough titration First Second Third Third titration titration titration titration Final burette reading: 19.00 34.05 20.86 36.01 23.57 (mL) Initial burette reading: (mL) 19.00 19.07 5.76 21.02 8.54 14 -98 is.ld 14.99 15.0g The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used in each titration is 14.80 mL. (1) Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations and reasoning.7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?Which of the following is the correct net ionic equation for this reaction? H3PO4(aq) + 3NaOH(aq) --> Na3PO4(aq) + 3H2O(l) (A) H+(aq) + OH–(aq) --> H2O(l) (B) 3Na+(aq) + PO43–(aq) --> Na3PO4(aq) (C) PO43–(aq) + 3NaOH(aq) --> Na3PO4(aq) + 3OH–(aq); (D) H3PO4(aq) + 3OH–(aq) --> 3H2O(l) + PO43–(aq)
- 24. A buffer is prepared using acetic acid, CH3COOH, (a weak acid) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 135.0 mL Concentration of CH3COOH(aq): 1.014 M Volume of CH3COONa(aq): 123.0 mL Concentration of CH3COONa(aq): 1.204 M What is the concentration of the conjugate base, CH3COO-, component in the final buffer solution? Give your answer in M, with correct significant digits.Given the equation: Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq) ?f=2.00×10^7 determine the concentration of NH3(aq) that is required to dissolve 295 mg of AgCl(s) in 100.0 mL of solution. The ?sp of AgCl is 1.77×10^−10. I've worked this through several times, but I am just not coming up with the right answer! Thanks :)Consider the following reactions: Reaction 1: HCIO, + KOH → KC1O, + H;O Reaction 2: HC;H;O2 + KOH → KC;H;O2+ H;O In both reactions, 15.00 mL of 0.8116 M acid is titrated with 0.4217 M KOH. A volume of 28.87 mL of KOH is required to reach the equivalence point in both reactions. a) What is the pH of the HC1O, solution before the titration has started? (No KOH has been added.) b) What is the initial pH of HC;H;O2 solution before the titration has started? K= 6.46 x 10-5 (Ok to use x is small.) c) What is the pH of Reaction 1 at the equivalence point? d) What is the pH of Reaction 2 at the equivalence point? e) What is the pH of Reaction 1 after 32.00 mL of KOH has been added? f) What is the pH of Reaction 2 after 18.00 mL of KOH has been added?