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![Cost- +H. Heon + 6H HNO + H2o Not Hot CH3 NH3 + H₂O - CH₃NH₂ + thot uPous- & What Hapon + NH3 D © Lloy(6.60023) = 13.64] (OH)](http://img.homeworklib.com/questions/76dbc2c0-d850-11eb-bcf5-ed4312692aca.png?x-oss-process=image/resize,w_560)
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1 Answer the following questions (a)...
Can someone help me? Did I do these two correctly? 1. Consider the reaction: conjugati bile...
Can someone help me? Did I do these two correctly?
1. Consider the reaction: conjugati bile acid base conjugale conjugate acid HNO3(aq) + H2O(1)=H30*(aq) + NO2 (aq). Label the species that is a acid/base and conjugate acid/base. 2. The pH of a solution at 25°C in which [OH) = 3.7 x 10 Mis: 10-14 3.7x10-6 -2.70 x10 20 M Pt--log C++] = 19.6 unter until the pH of the solution is 11.50. The
if someone could show me how to do all of these, that would be great Acids...
if
someone could show me how to do all of these, that would be
great
Acids and Bases Name Directions: Answer/Calclulate the following. Use a separate sheet if needed. Give the Arrhenius and Bronsted/Lowry definitions for acids and bases. How are they similar and different? In the Bronsted/Lowry definition, acids and bases always occur If an equation is "looked at in reverse", then the acid becomes the -. These are known and the base becomes Identify the acid, base, conjugate...
Which one of the following salts, when dissolved in water, produces the solution with the highest...
Which one of the following salts, when dissolved in water, produces the solution with the highest pH? HINT: Remember that BASES have high pH. Mgo CH3NH31 LICIO4 O NaHSO4 Which of the following are weak diprotic acids? hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4 carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3COOH O carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3 formic acid - HCOOH, acetic acid...
1. Determine if the following salt is neutral, acidic or basic. If acidic or basic, write...
1. Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. Ba(CHO₂)₂ 2. Write the formula of the conjugate base of the Brønsted-Lowry acid, HC₂O₄⁻ 3. What is the pH of a 0.0880 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)? 4. What is the pH of a...
could someone help me with 15.25 and 15.27 and 15.32 please? $13 Write of the conjugate...
could someone help me with 15.25 and 15.27 and 15.32 please?
$13 Write of the conjugate acid of substances. (The information in Tables 15.6 10/26/2019 the following substances. (The infor and 15.8 may be helpful.) (a) hydrogen sulfate ion (c) ammonia (b) water (d) pyridine he formula and name for the conjugate base of the substances. (The information in Tables 15.6 and 15.24 Writer 15.25 Write the form following substances. (The int 15.8 may be helpful.) (a) nitric acid (b)...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
Hi.can you help me answer questions b and d.thanks a lot for your help Elm in...
Hi.can you help me answer questions b and d.thanks a
lot for your help
Elm in the pH of a buffer solution which contoing 9.60 mole Of ammonium nitrate and 0.4 0 mole of ammonig in a 1.0 d m 3 solution. Given Ra for NH 4 = 5.6x 10-10 Lo Write the acid-base conjugate pairs for the following reaction N H 4 + H2O2 N H + HOÁ (2 marks) nicolculate the pH of 0.75 M. Sodium Qietate Solution...
Hey! Can you please help me with the following two questions I am highly confused and...
Hey! Can you please help me with the following two questions I am highly confused and I don't really understand them at all. Thank you!! 16, Please help me with them, we have a test this thursday and problems that are similar are supposed to be on there. Thank you so much!!! 1.The pH of a 0.14-M solution of phthalic acid (H2C8H4O4) is measured to be 1.91. Use this information to determine a value of Ka for phthalic acid. H2C8H4O4(aq)...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
Can someone help me? Did I do these two correctly?
1. Consider the reaction: conjugati bile acid base conjugale conjugate acid HNO3(aq) + H2O(1)=H30*(aq) + NO2 (aq). Label the species that is a acid/base and conjugate acid/base. 2. The pH of a solution at 25°C in which [OH) = 3.7 x 10 Mis: 10-14 3.7x10-6 -2.70 x10 20 M Pt--log C++] = 19.6 unter until the pH of the solution is 11.50. The
if
someone could show me how to do all of these, that would be
great
Acids and Bases Name Directions: Answer/Calclulate the following. Use a separate sheet if needed. Give the Arrhenius and Bronsted/Lowry definitions for acids and bases. How are they similar and different? In the Bronsted/Lowry definition, acids and bases always occur If an equation is "looked at in reverse", then the acid becomes the -. These are known and the base becomes Identify the acid, base, conjugate...
Which one of the following salts, when dissolved in water, produces the solution with the highest pH? HINT: Remember that BASES have high pH. Mgo CH3NH31 LICIO4 O NaHSO4 Which of the following are weak diprotic acids? hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4 carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3COOH O carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3 formic acid - HCOOH, acetic acid...
could someone help me with 15.25 and 15.27 and 15.32 please?
$13 Write of the conjugate acid of substances. (The information in Tables 15.6 10/26/2019 the following substances. (The infor and 15.8 may be helpful.) (a) hydrogen sulfate ion (c) ammonia (b) water (d) pyridine he formula and name for the conjugate base of the substances. (The information in Tables 15.6 and 15.24 Writer 15.25 Write the form following substances. (The int 15.8 may be helpful.) (a) nitric acid (b)...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
Hi.can you help me answer questions b and d.thanks a
lot for your help
Elm in the pH of a buffer solution which contoing 9.60 mole Of ammonium nitrate and 0.4 0 mole of ammonig in a 1.0 d m 3 solution. Given Ra for NH 4 = 5.6x 10-10 Lo Write the acid-base conjugate pairs for the following reaction N H 4 + H2O2 N H + HOÁ (2 marks) nicolculate the pH of 0.75 M. Sodium Qietate Solution...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
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