ph_calculations.pdf | |
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March Week 2-3-4: Acids and Bases
Learning Target: Learning Target: C5.7A Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II. C5.7B Predict products of an acid-base neutralization. C5.7C Describe tests that can be used to distinguish an acid from a base. C5.7D Classify various solutions as acidic or basic, given their pH. C5.7E Explain why lakes with limestone or calcium carbonate experience less adverse effects from acid rain than lakes with granite beds. C5.7f Write balanced chemical equations for reactions between acids and bases and perform calculations with balanced equations. C5.7g Calculate the pH from the hydronium ion or hydroxide ion concentration. C5.r7i Identify the Brønsted-Lowry conjugate acid-base pairs in an equation. (recommended) C5.7h Explain why sulfur oxides and nitrogen oxides contribute to acid rain.]
Read, Take Notes and Check your Understanding.
P. 530: Look at figure 1. Give examples of acids.
P. 531: Explain how acid solution conduct electricity.
Explain how acids react with zinc metals in figure 3.
P. 532: Define strong acid. Give two examples from table 1.
Define strong base. Give two examples from table 1.
Describe Figure 4. what is a hydronium ion?
P. 533: Table 2. Give two examples of strong bases and weak bases.
Figure 5: list some of the basic products found at home.
P. 534: Define strong base, weak base.
Figure 6: Explain why sodium hydroxide is a strong base. Why is ammonia a weak base?
P. 535: Define Bronsted-Lowry acid
Figure 7. Explain how hydrogen chloride is a representative of Bronsted-Lowry acid.
P. 536: Define Bronsted-Lowry base.
Write the equilibrium equation of ammonia in water.
P. 537: Define Conjugate acid, conjugate base.
Table 3; Give two examples of conjugate acid-base pair.
P. 538: Define amphateric.
Explain how hydrogen carbonate ion (HCO3-) is amphoteric in aqueous solutions.
P. 539: Figure 9. Explain how water is both an acid and a base. Write the equilibrium reaction.
P. 540: Figure 10. Explain the relationship between the concentration of OH- and H3O+.
What is the self-ionization constant of water Kw.
P. 541: Do sample problem A. Do practice problems 1, 2, 3, 4 and 5.
P. 540: Redo the calculation for the concentration of OH- for each solution.
P. 542: Define neutral solution, pH.
P. 543: Skills toolkit.
Learn how to calculate pH from the concentration of H3O+ using the calculator.
Learn how to calculate H3O+ from pH using the calculator
P. 544: Read sample problem B. Do practice problems 1, 2, 3, 4.
P. 542: Recalculate the pH of the solutions.
Write the equation for pH and for the hydronium ion.
P. 545: Do sample problem C. Do practice problems 1, 2, 3, 4.
P. 546: Figure 12. List the different compounds, the pH of each compound and whether it is acidic or basic.
P. 547: What is a pH meter?
P. 548: Define neutralization reaction.
Explain how the pH and color of the indicator change in the neutralization reaction.
P. 549: Write down the neutralization reaction.
Explain the products of the neutralization reaction in figure 16.
P. 550: Define: equivalence point, titration, titrant, standard solution.
P. 554: Define: transition range, end point.
Copy table 6
P. 555: Write the formula for titration
Read Sample Problem D
P. 556: Do practice problems 1 2, 3,,and 4.
Learning Target: Learning Target: C5.7A Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II. C5.7B Predict products of an acid-base neutralization. C5.7C Describe tests that can be used to distinguish an acid from a base. C5.7D Classify various solutions as acidic or basic, given their pH. C5.7E Explain why lakes with limestone or calcium carbonate experience less adverse effects from acid rain than lakes with granite beds. C5.7f Write balanced chemical equations for reactions between acids and bases and perform calculations with balanced equations. C5.7g Calculate the pH from the hydronium ion or hydroxide ion concentration. C5.r7i Identify the Brønsted-Lowry conjugate acid-base pairs in an equation. (recommended) C5.7h Explain why sulfur oxides and nitrogen oxides contribute to acid rain.]
Read, Take Notes and Check your Understanding.
P. 530: Look at figure 1. Give examples of acids.
P. 531: Explain how acid solution conduct electricity.
Explain how acids react with zinc metals in figure 3.
P. 532: Define strong acid. Give two examples from table 1.
Define strong base. Give two examples from table 1.
Describe Figure 4. what is a hydronium ion?
P. 533: Table 2. Give two examples of strong bases and weak bases.
Figure 5: list some of the basic products found at home.
P. 534: Define strong base, weak base.
Figure 6: Explain why sodium hydroxide is a strong base. Why is ammonia a weak base?
P. 535: Define Bronsted-Lowry acid
Figure 7. Explain how hydrogen chloride is a representative of Bronsted-Lowry acid.
P. 536: Define Bronsted-Lowry base.
Write the equilibrium equation of ammonia in water.
P. 537: Define Conjugate acid, conjugate base.
Table 3; Give two examples of conjugate acid-base pair.
P. 538: Define amphateric.
Explain how hydrogen carbonate ion (HCO3-) is amphoteric in aqueous solutions.
P. 539: Figure 9. Explain how water is both an acid and a base. Write the equilibrium reaction.
P. 540: Figure 10. Explain the relationship between the concentration of OH- and H3O+.
What is the self-ionization constant of water Kw.
P. 541: Do sample problem A. Do practice problems 1, 2, 3, 4 and 5.
P. 540: Redo the calculation for the concentration of OH- for each solution.
P. 542: Define neutral solution, pH.
P. 543: Skills toolkit.
Learn how to calculate pH from the concentration of H3O+ using the calculator.
Learn how to calculate H3O+ from pH using the calculator
P. 544: Read sample problem B. Do practice problems 1, 2, 3, 4.
P. 542: Recalculate the pH of the solutions.
Write the equation for pH and for the hydronium ion.
P. 545: Do sample problem C. Do practice problems 1, 2, 3, 4.
P. 546: Figure 12. List the different compounds, the pH of each compound and whether it is acidic or basic.
P. 547: What is a pH meter?
P. 548: Define neutralization reaction.
Explain how the pH and color of the indicator change in the neutralization reaction.
P. 549: Write down the neutralization reaction.
Explain the products of the neutralization reaction in figure 16.
P. 550: Define: equivalence point, titration, titrant, standard solution.
P. 554: Define: transition range, end point.
Copy table 6
P. 555: Write the formula for titration
Read Sample Problem D
P. 556: Do practice problems 1 2, 3,,and 4.
answers_to_practice_problems_page_541.pdf | |
File Size: | 270 kb |
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answers_to_practice_problems_b_page_544.pdf | |
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answers_to_practice_problems_c_in_page_545.pdf | |
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answers_to_practice_problems_d_in_page_556..pdf | |
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March Week 1: Molarity
Learning Target: Define molarity and calculate the molarity of a solution.
Read, Take Notes and Check your Understanding.
P. 454-455: Define: solution, solvent, and solutes.
P. 462: Define molarity.
P. 464. Write the equation for molarity.
P. 462: Define molarity
P. 465: Read Sample Problem B. Do Practice 1, 2, 3, 4 and 5.
Molar mass of CH3COOH = 60.05196 g/mol
Molar mass of HCl = 36.46094 g/mol
Molar mass of H2SO4 = 98.07848 g/mol
Molar mass of AgNO3 = 169.8731 g/mol
Molar mass of Ba(OH)2 = 171.34168 g/mol
P. 457: List the methods for separating mixtures.
P. 466: Read Sample Problem C.
Do practice problems 1, 2, 3.
Molar mass of ZnCl2 = 136.286 g/mol
Molar mass of Cds = 144.46 g/mol
P. 489: Do 47, 48, 50, 51, 52, 53, 54
Learning Target: Define molarity and calculate the molarity of a solution.
Read, Take Notes and Check your Understanding.
P. 454-455: Define: solution, solvent, and solutes.
P. 462: Define molarity.
P. 464. Write the equation for molarity.
P. 462: Define molarity
P. 465: Read Sample Problem B. Do Practice 1, 2, 3, 4 and 5.
Molar mass of CH3COOH = 60.05196 g/mol
Molar mass of HCl = 36.46094 g/mol
Molar mass of H2SO4 = 98.07848 g/mol
Molar mass of AgNO3 = 169.8731 g/mol
Molar mass of Ba(OH)2 = 171.34168 g/mol
P. 457: List the methods for separating mixtures.
P. 466: Read Sample Problem C.
Do practice problems 1, 2, 3.
Molar mass of ZnCl2 = 136.286 g/mol
Molar mass of Cds = 144.46 g/mol
P. 489: Do 47, 48, 50, 51, 52, 53, 54
answers_for_practice_problems_b_in_page_465.pdf | |
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answers_to_section_review_page_467.pdf | |
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answers_to_page_870__concentration_and_molarity_.pdf | |
File Size: | 150 kb |
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