Concept explainers
Interpretation:
The reason for the higher pH value of
Concept Introduction:
A base is defined as the substance that can give
If the concentration of
The acidic and basic nature of the solution can be expressed in terms of pH of the solution. The range of pH lies from 0 to 14. The pH value from 0 to 7 indicates an acidic solution whereas the pH value from 7 to 14 stands for a basic solution. A neutral solution can be expressed as pH 7. It can be calculated with the help of concentration
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Chapter 9 Solutions
CONNECT IA GENERAL ORGANIC&BIO CHEMISTRY
- 3 How to Titrate: Lab Techniques Titration Titration Procedures: Add about 100mL of a 0.1 M NAOH solution to a 250mL beaker. 2. Obtain a buret and rinse with about 10 ml of the NaOH solution. 3. Fill the buret with NaOH and record starting volume to the nearest 1m" of a milliliter. 4. Measure out exactly 10.0 ml of HC in a graduated cylinder and add it to a 250mL Erlenmeyer flask along with 1 drop of phenolphthalein indicator. 5. Slowly add the NaOH to the flask with the acid and swirl. Continue adding the base until a color change (faint pink) occurs and remains for at least 10 seconds. This is the endpoint of this neutralization eaction. 6. Read and record the ending volume of NaOH in the buret, 7. Repeat steps 1 through 6 two more times for Trials 2 and 3. 8. Calculate the volume of base added in each trial. 9. Use the volume of base added and the volume of acid added to calculate the molarity of the acid for each trial. 10. Calculate the average molarity of the acid. 11. Calculate…arrow_forwardWhat is the percent dissociation of 0.150 M triethylamine? (The Kb value for triethylamine is 5.25 × 10-4.) a. 5.92 %b. 5.75 %c. 39.4 %d. 5.75 x 10-30 %arrow_forwardHow many moles and grams of Ca(OH)2 are needed to neutralize 25.0 mL of 0.100 M HNO3? (Given: MHNO3 = 63.01 g.mol-1; MCa(OH)2 = 74.1 g.mol-1).arrow_forward
- What are the K1 and K2 (dissociation constants)? Given... Molarity NaOH: .3, Concentration of unknown: 31 g/L # mL NaOH to reach 1st inflection point: 25 (pH 4) # mL NaOH to reach 2nd inflection point: 50 (pH 11) pH @ 1st 1/2 equivalence point: 2.6arrow_forwardManganese carbonate (MnCO3) has low solubility in neutral water (8 mg/L), but dissolves completely in water when pH is low. While there is no obvious common ion effect, it does have a distinct solubility relationship. Propose a brief explanation. (2-4 sentences max)arrow_forward3- The concentration of a solution containing 5 ng of KCI in 200 mg water is : (0.025 ppt, 0.025 ppm, 0.025 ppb ). 4- Which of these values are representing strongest acid (Keg= 5X 108, Keq = 5 x 10. Keq= 1,8 x 10 2) 5- Which of the following values represent the less soluble : (Ksp = 1 x 10 $ , Ksp = 7X 1011, Ksp =5X105 Ksp= 3 x1011 ).arrow_forward
- 0 20.00 mL of a H₂SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint with 40.05 mL of a 0.1155 M NaOH solution. What is the concentration of the H₂SO4 solution? [H₂SO₁] = Marrow_forwarda. What is the percent ionization in 0.80 M NH3 (Kb Percent ionization = % % = % 1.8 × 10-5)? b. What is the percent ionization in 0.090 M NH3 (Kb Percent ionization = c. What is the percent ionization in 1.0 M CH3NH₂ (Kb = 4.38 × 10¯4)? Percent ionization = = 1.8 × 10-5)?arrow_forwardWhat is the pH of a solution composed of 0.20 M NH3 and 0.15 M NHẠC1? (Pkb of NH3-4.75) O 2.15 4.62 6.16 9.38 not responsible for thearrow_forward
- 5. a) The Kw value that we normally use is for room temperature (25°C). Calculate the equilibrium H+ concentration and pH of pure, neutral water at 0.0°C (Kw= 1.14 x 10-15at 0.0°C) b) Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution.(Kb= 4.37 x 10-4at 25°C)arrow_forward3. Calculate the number of moles a. 1.0 mL 0.10M Pb(NO3)2 and 5.0 mL, 0.10 M KI b. 2.0 mL 0.10M Pb(NO3)2 and 4.0 mL, 0.10 M KIarrow_forwardA 700.0 mL solution is 0.209 M CH₂CH₂CH₂COOH (K₁-1.5 x 10%) and 0.253 M NaCH-CH₂CH₂COO. What is the pH after the addition of 5.00 mL of 0.750 M NaOH? (4) 4.76 B) 4.93 4.89 4.72arrow_forward
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- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
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