mL of a 0.530M C2H5NH2 solution (Kb ver should be entered with 3 significant figures; do not enter units; give answer in normal notation-examples include 1.2 123. and 12.3)
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- Given three acid-base indicators—methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)—which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acidFifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. How many milliliters of 12 M HCI must be added to 0.500 K of the original solution to change its pH to 9.00?
- A 0.100 L solution is composed of 0.500 M (CH3)2NH and 0.500 M (CH3)2NH2Cl at 25 oC. What is the pH of the solution after 0.010 moles of KOH are added to the solution at the same temperature?You may assume there is no change in volume for the system. Enter your answer with two decimal places.At 25 degrees C: Kb for (CH3)2NH = 5.9 x 10-4Calculate the pH of a solution containing 23 mL of 1.54 M of a weak weak base B OH, like NH4OH, or simply written as NH3, titrated with 17 ml of 1.01 M a strong acid AH, for instance HCl. The base dissociation constant, Kb , is 1.00e-5. pH ← please insert your valueWhat is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10-5) when 100.0 mL of a 0.0.75 M HCl solution is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ?Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.
- Walter White requires a sulfuric acid (Strong acid) solution to use in a very important synthetic reaction. He finds a bottle labeled H2SO4, but by some strange turn of events, he cannot remember the concentration. He decides to perform a titration to determine the concentration of the H2SO4. He pours 22.20 mL of his unknown sulfuric acid solution into a flask and finds that it requires 29.50 mL of 0.57 M KOH (strong base) to reach the endpoint. What is the concentration of Walter White's sulfuric acid solution? (Enter your numeric answer only, do not use scientific notation, enter 2 decimal places with your answer) For reference: KOH = 56.106g/mol H2SO4= 98.079g/mol Avagadro's number 6.022x1023A group of students perform a titration experiment. The buret tube is filled to the 0.00ml line with 0.100M NaOH solution. The E. flask contains 50.0ml ov 0.100M HC2H3O2 solution. The Ka of the acetic acid is: Ka = 1.8 x 10-5. A. Draw a simple diagram of the apparatus, label parts and label the solution in each part. B. What volume of NaOH is added to reach the equivalence point? C. Write the ionization equation for the acid. D. Write the ionic equation for the conjugate acid reacting with water. One product is the OH- polyatomic ion. E. What is the pH at the equivalence point?A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2(ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 what is the pH at the equivalent point?
- From the titrations below, calculate the molarity of the NaOH solution in each of the following? Make sure you balance the equations. a.) NaOH + HCl => NaCl + H2O 32.00ml of NaOH is required to completely react with 25.00ml of 0.150 M HCl. b.) NaOH + H2SO4 => Na2SO4 + H2O 42.00 ml of NaOH is required to completely react with 18.00ml of 0.10M H2SO4.Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base:(a) 0 mL(b) 25.00 mL(c) 39.00 mL(d) 39.90 mL(e) 40.00 mL(f ) 40.10 mL(g) 50.00 mL Use the values obtained to sketch a curveof [H₃O⁺] vs. mL of added titrant. Are there advantages or dis-advantages to viewing the results in this form? Explain.Calculate the pH at the equivalence point of 61 ml solution containing a weak base, BOH, for instance NH4OH, often written as NH3 , titrated with 20 ml of a strong acid, HA , like HCl, with a concetration of 1.1 M. The base dissociation constant, Kb , is 1.60e-7. pH ← please insert your value