Write the equilibrium expressions, charge balance equation, and the mass balance equations for 0.100 M aqueous HO2CCO2H and show that the number of equations you list is equal to the number of unknowns in the solutions. Hint: Do not forget the auto protolysis of water.
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Write the equilibrium expressions, charge balance equation, and the mass balance equations for 0.100 M aqueous HO2CCO2H and show that the number of equations you list is equal to the number of unknowns in the solutions. Hint: Do not forget the auto protolysis of water.
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- The reaction just described is reversible. Deprotonation of the conjugate acid of an organic base by water provides another example of simultaneous making and breaking of sigma bonds. Thus, in the deprotonation of anilinium ion by water, the base is water, which has unshared electrons on the ________ atom. The acid is ________ ion. A pair of ________ electrons on the oxygen atom of water is pushed toward the ________ atom. Simultaneously, the pair of ________ electrons between the hydrogen and ________ atom of the anilinium ion is pushed toward the ________ atom. Thus, the oxygen- ________ sigma bond is made and a hydrogen- ________ sigma bond is broken. The nitrogen atom, which possessed a positive charge, is now ________, and the oxygen atom, which was neutral, now possesses a formal ________ charge.Calculate the hydrogen-ion concentration and the pH of a solution of 0.0001M H2CO3, and also calculate what fraction of the H2CO3 has been dissociated. Compare this fraction with the fraction dissociated when the concentration is 0.01M (given that the pH is 4.2 in a 0.01M solution). What generalization can you make regarding the effect of dilution on the degree of dissociation?Answer question 5&6. Give only the important solutions.
- Identifying the major species in weak acid or weak base... The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. acids: 1 mol of NaOH is added to 1.0 L of a 0.7M HCN bases: O solution. other: O 0.3 mol of NaOH is added to acids: 1.0 L of a solution that is bases: O 0.8M in both HCN and NaCN. O other:Calculate the equilibrium concentration of carbonate in a 0.067 M solution of carbonic acid. Do not enter units as part of your answer. Use “E” for scientific notation.Identifying the major species in weak acid or weak base... The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. acids: 1.9 mol of KOH is added to 1.0 L of a 1.0M HCN bases: solution. O other: 0.095 mol of HNO, is added O acids: to 1.0 L of a solution that is bases: 1.4M in both HCN and KCN. O other: O O D O O D
- (References] This question has multiple parts. Work all the parts to get the most points. Use the References to access important values if needed for this question. The [OH ] of a solution can be determined from the pOH using the equation: [OH] = 10-POH Where: [OH]= hydroxide ion concentration a Use the rules for logarithms and exponents to solve for pOH in terms of [OH ]. NOTE: Capitalization counts. pOH= Submit Submit Answer Retry Entire Group 4 more group attempts remaining Previous NextPredicting acid or base strength from the conjugate Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. Explanation species F HCIO, C102 HIO HF OH H₂O IO Check relative pH of 0.1 M aqueous solution (Choose one) ▼ to 1 (lowest) (Choose one) ▼ (Choose one) 2 (Choose one) ▼ 4 7 Search S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center AAfter hydrolysis of salt in aqueous solution is always a basic solution. O True False
- Predicting acid or base strength from the conjugate Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CH₂CH(OH) COOH Explanation H₂O C6H5NH3 OH C6H5O CHẠNH, CHOK CH₂CH(OH)COO Check relative pH of 0.1 M aqueous solution (Choose one) 4 2 (Choose one) ▼ (Choose one) ▼ (Choose one) ▼ 3 5 Q Search X 1/5 3 - Allie V ?圖 allo Ar © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center…Predicting acid or base strength from the conjugate Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. Explanation species CH₂COOH OH 103 CH3COO HONH, H₂O HIO3 HONH, Check relative pH of 0.1 M aqueous solution 2 8 (highest) 5 (Choose one) ▼ (Choose one) ▼ (Choose one) ▼ (Choose one) ▼ 3 ▬▬ Q Search X S 4 ?圖 l Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessibilitySelect the correct answers: “Ocean acidification is a process that occurs when atmospheric carbon dioxide dissolves in the ocean and is subsequently converted into (methane; carbonic acid; carbonate ions; sodium carbonite) . This then causes the pH of the ocean to (increase; decrease; fractionate; multiply) and become more acidic.”
