Homework Answers
Both acids and bases produce ions in solutions.
i. Base solutions: Common constituent in all basic solutions is OH- ions
ii. Acidic Solutions:Common constituent in all acidic solutions is H+ ions
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What is the common constituent in all base and acids solutions? i. Base solutions: ii. Acid...
a Many laboratories keep bottles of 1.0 M solutions of the common acids on hand. Given...
a Many laboratories keep bottles of 1.0 M solutions of the common acids on hand. Given 12.1 M of the concentrated acid HCl, determine how many milliliters of concentrated acid would be required to prepare 196 mL of a 1.0 M solution of the acid. mL b Many laboratories keep bottles of 1.0 M solutions of the common acids on hand. Given 15.9 M of the concentrated acid HNO3, determine how many milliliters of concentrated acid would be required to...
Part 2 (acid/base) 4. Consider the following questions about acids and bases. a) Which of these...
Part 2 (acid/base) 4. Consider the following questions about acids and bases. a) Which of these solutions will have the highest concentration of OH ions? Which will have the lowest? i) 0.60 M CH3NH2 ii) 0.25 M Sr(OH) iii) 0.35 M LiOH) b) Predict the product of the following reaction. Make sure the reaction is balanced. Na)+Ba(OH) (ag) c) Write a net ionic equation for b) d) Identify the acid and the base in the following reaction (remember the Bronsted...
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2....
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2. Which species is the conjugate base of HPO 2-? Refresher of Acid/Base Equilibria, Ka, and pK., and buffer solutions: 1. The (H30') in a cabernet Sauvignon wine is 5.9 x 10 M. What is the (-OH) in this wine? 2. The pH of a lime is 1.90. What is the [H30*]? 3. What is the pH of a cleaning solution with a [H3O+] =...
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M...
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M propionic acid, K. = 1.3*10% ii) 0.0085 M phenol, K. = 1.3*100 b) Calculate the pH of 0.1 M sulfuric acid, being a strong acid for giving away the first H', and K, for the second step is 1.2*10? (2 points) c) Calculate the pH of a 0.1 M aqueous solution of NaCN. NaOH is a strong base, while the K. of HCN is...
Paragraph k acids and bases. We need to we will be working with solutions of both strong acids an...
Paragraph k acids and bases. We need to we will be working with solutions of both strong acids and bases, and wea good idea of what compounds are actually present in these solutions before we begin. Write an equation for the solution that results when each compound is placed in water. For the ionic compounds, there will be a second hydrolysis equation that takes place. Make sure that you use single arrows to represent full extent reactions, and double arrows...
Bicarbonate (HCO3-) is a common water quality constituent. Bicarbonate dissociates as a weak acid to give...
Bicarbonate (HCO3-) is a common water quality constituent. Bicarbonate dissociates as a weak acid to give carbonate (CO32-) as follows: HCO3- = CO32- + H+ pKa = 10.33 Determine whether HCO3-, or CO32-, is predominant in natural waters at pH = 7.90. I got (HCO_3)^- ; I would just like to double check!
I missed class and a classmate sent her notes over and I am confused on what the notes in purple ...
I missed class and a classmate sent her notes over and I am
confused on what the notes in purple mean.
General Chemistry II Module 6 Chapter 16: Aqueous lonic Equilibrium 16.2 Buffers: Solutions That Resist pH Change 1. What is a buffer? significant amounts of weak acids and its conjugate base. The weak acid in a buffer A buffer resists pH change by neutralizing added acid or base. Buffers contain neutralizes added base. The conjugate base in a buffer...
Designate the conjugate Brønsted-Lowry base for each of the following acids: (i) H2CO3 (ii) HNO3 (iii)...
Designate the conjugate Brønsted-Lowry base for each of the following acids: (i) H2CO3 (ii) HNO3 (iii) H+(aq)
Which of the following fatty acids is/are classified as omega-3 fatty acid? (I) only (II) only...
Which of the following fatty acids is/are classified as omega-3 fatty acid? (I) only (II) only (III) only (I) and (III) (II) and (III)
O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the following data on...
O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: base name formula acid name formula acetic acid HCH,CO2 1.8 x 10-5 nitrous acid HNO 4.5 x 10 ammonia NH; 1.8 x 10 ethylamine C,H, NH, 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH,...
a Many laboratories keep bottles of 1.0 M solutions of the common acids on hand. Given 12.1 M of the concentrated acid HCl, determine how many milliliters of concentrated acid would be required to prepare 196 mL of a 1.0 M solution of the acid. mL b Many laboratories keep bottles of 1.0 M solutions of the common acids on hand. Given 15.9 M of the concentrated acid HNO3, determine how many milliliters of concentrated acid would be required to...
Part 2 (acid/base) 4. Consider the following questions about acids and bases. a) Which of these solutions will have the highest concentration of OH ions? Which will have the lowest? i) 0.60 M CH3NH2 ii) 0.25 M Sr(OH) iii) 0.35 M LiOH) b) Predict the product of the following reaction. Make sure the reaction is balanced. Na)+Ba(OH) (ag) c) Write a net ionic equation for b) d) Identify the acid and the base in the following reaction (remember the Bronsted...
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2. Which species is the conjugate base of HPO 2-? Refresher of Acid/Base Equilibria, Ka, and pK., and buffer solutions: 1. The (H30') in a cabernet Sauvignon wine is 5.9 x 10 M. What is the (-OH) in this wine? 2. The pH of a lime is 1.90. What is the [H30*]? 3. What is the pH of a cleaning solution with a [H3O+] =...
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M propionic acid, K. = 1.3*10% ii) 0.0085 M phenol, K. = 1.3*100 b) Calculate the pH of 0.1 M sulfuric acid, being a strong acid for giving away the first H', and K, for the second step is 1.2*10? (2 points) c) Calculate the pH of a 0.1 M aqueous solution of NaCN. NaOH is a strong base, while the K. of HCN is...
Paragraph k acids and bases. We need to we will be working with solutions of both strong acids and bases, and wea good idea of what compounds are actually present in these solutions before we begin. Write an equation for the solution that results when each compound is placed in water. For the ionic compounds, there will be a second hydrolysis equation that takes place. Make sure that you use single arrows to represent full extent reactions, and double arrows...
I missed class and a classmate sent her notes over and I am
confused on what the notes in purple mean.
General Chemistry II Module 6 Chapter 16: Aqueous lonic Equilibrium 16.2 Buffers: Solutions That Resist pH Change 1. What is a buffer? significant amounts of weak acids and its conjugate base. The weak acid in a buffer A buffer resists pH change by neutralizing added acid or base. Buffers contain neutralizes added base. The conjugate base in a buffer...
Which of the following fatty acids is/are classified as omega-3 fatty acid? (I) only (II) only (III) only (I) and (III) (II) and (III)
O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: base name formula acid name formula acetic acid HCH,CO2 1.8 x 10-5 nitrous acid HNO 4.5 x 10 ammonia NH; 1.8 x 10 ethylamine C,H, NH, 6.4 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH,...
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