PRE-LAB DATA SHEET
1 |
2 |
3 |
4 |
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Initial number of moles |
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HAn(aq) |
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OH-(aq) |
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Number of moles at equilibrium |
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HAn(aq) |
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An-(aq) |
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Equilibrium concentrations, mol/L |
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HAn(aq) |
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An-(aq) |
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H3O+(aq) |
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Ka |
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Average Ka |
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Which of the weak acids in Table 1 do you think your unknown acid is?
A student following the procedure in this lab prepared 4 solutions by adding 12.00, 23.00, 26.00,...
I'm having trouble with the calculations for my chemistry lab: Determination of an Acid Dissociation Constant, Ka Half-Neutralization Molarity of acetic acid: 2 M Molarity of NaOH: 1 M Volume of acetic acid: 25 mL NaOH Solution Final Buret Reading: 6.23 mL Initial Buret Reading: 0.01 mL Volume added: 6.22 mL Total Volume of Solution: 250 mL pH: 3.85 Caculating Ka Initial number of moles HAn: ? OH-: ? Number of moles at equilibrium: HAn: ? An-: ? Equilibrium concentrations,...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
17. From the following equilibrium process involving a weak acid (K2), derive the Henderson Hausselbach equation. (show all work) HA(aq) + H2O(lig) + H3O+(ag) + A (ag) 18. If the value of Ka for HCN is 4.9 x 10-10, calculate the equilibrium constant for CN-ag) +H2O(lig) H HCN(aq) + OH(aq) 19. Briefly justify the acidity difference in the following oxyacids: HCIO, HC102, and HC103. 20) What is the pH of a solution made by mixing 100.00 mL of 0.20 M...
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic acid with 0.100 M NaOH and monitored the titration with a pH meter. His titration data were: Volume of NaOH solution added, mL /// pH 0.00 | 3.30 2.00 | 4.22 4.00 | 4.55 6.00 | 4.76 8.00 | 4.92 10.00 | 5.06 12.00 | 5.18 14.00 | 5.29 16.00 | 5.40 18.00 | 5.51 20.00 | 5.62 22.00 | 5.74 24.00 | 5.88...
B. pH of Buffer Solutions Follow the instruction in the lab book for making the buffer solution. Mass of NaCHC003H20 (FN= 136 g/mhol)--2209___ Moles of CH3COO Concentration of CH3COOH Volume of CH3COOH (mL) Moles of CH3COOH .OML o22 nol Analysis of Buffer Solution Measured pH of Buffer Solution Calculated pH of Buffer Solution (show work) 1. [conjugate base] weak acid to calculate the pH.
1. Determine the number of moles of reagent in the following solutions: a. 25.00 mL of 0.10 M acetic acid b. 5.55 mL of 0.092 M NaOH C. 0.50 mL of 0.087 M HCI 2. A buffer solution contains 0.120 M acetic acid and 0.150 M sodium acetate. a. How many moles of acetic acid and of sodium acetate are present in 50.0 mL of solution? b. If we add 5.55 mL of 0.092 M NaOH to the solution in...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you! Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
9) Which one of the following pairs cannot be mixed together to form a buffer solutions A) KOH, HNO2 B) H2S03. KHSO3 C) HONH2, HONH3CI D) NaCI, HCI E) RbOH, HF 10) The Henderson-Hasselbalch equation is acid) acid] A) pH- pKa log basel base] D) pH - pKaobase [acid 11) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A- A) A (aq) H30+ (aq) HA (aq) H20 0) B) HA (aq) + OH-(aq) 근...