Since only salt NaA and H2O present in the solution so H+ ion comes from hydrolysis...
Since only salt NaA and H2O present in the solution so H+ ion comes from hydrolysis of NaA to give NaOH and HA and dissociation of H2O. Hence we calculate pH by formula for salt formed by weak acid and strong base.
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Since only salt NaA and H2O present in the solution so H+ ion
comes from hydrolysis...
Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH)...
Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example:...
what is the predominant solute ion or molecule (A-, OH-, H+, or HA) present in a...
what is the predominant solute ion or molecule (A-, OH-, H+, or HA) present in a solution of weak acid? what is the molar ratio of HA (weak acid) ans A- (its conjugate base) when 50% of a weak acid has been neutralized by a strong base?
The pH of an aqueous solution of the salt Na SO, (sodium sulfate) will a) be...
The pH of an aqueous solution of the salt Na SO, (sodium sulfate) will a) be basic (because it is a weak acid-strong base salt) b) be acidic (because it is a strong acid-weak base salt) c) be neutral (because it is a strong acid-strong base salt) d) not be known (because it is a weak acid-weak base salt) e) no correct response
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present...
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion O water sodium ion O acetate ion When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion water O sodium ion acetate non aer 20191121-WA0036.jpg Question 9 If the pH of a salt solution is 5.3, the salt must be...
During the titration the following reaction occurs HA + NaOH = NaA+H2O What is the concentration...
During the titration the following reaction occurs HA + NaOH = NaA+H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? M Use [A] and the pH at the equivalence point to estimate Ko of the weak acid (this is the hard way of estimating K.) Use the pH at the half-way point to estimate of the weak acid (this is the easier way) Your grade will be shown after clicking 'Grade'...
If a small amount of a strong base is added to a buffer made up of...
If a small amount of a strong base is added to a buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because A.CH3COOK or NaOH B.CH3COOK only C.NaOH only D.NH4Cl only E.NaCl or CH3COOK
Acid base equalibria Solution E is made by mixing 1o mL NaA stock solution. e. .H...
Acid base equalibria
Solution E is made by mixing 1o mL NaA stock solution. e. .H stk solution and 10 .c ml Calculate the [HA]o by dilution of the HA stock solution. Calculate (AJ, by dilution of the NaA stock solution. Calculate [H'Je from the pli. 53 25 From the stoichiometry calculate [A]eq and [HAI Using the values above, calculate K, for the weak acid HA. f. Solution F is made by mixing 2.00 mL HA stock solution and 2o...
help with these chemistry questions 1. Explain what happens to the concentration of H,O' ions in...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
questions are in red Consider the following salt solutions: (i) NH4Cl – NH+ + C- Notice...
questions are in red
Consider the following salt solutions: (i) NH4Cl – NH+ + C- Notice that as a salt, NH,Cl dissociates completely in solution. So, what are the parents of this salt? The cation, NH, in this case, is from the base obtained by adding enough OHto balance the positive charge(s) on the cation; Viz, NH,OH. Similarly, the anion, Cl. comes from the acid. So the parent acid can be obtained by adding enough Hi to neutralize the charge...
The pH of an aqueous solution of the salt Na SO, (sodium sulfate) will a) be basic (because it is a weak acid-strong base salt) b) be acidic (because it is a strong acid-weak base salt) c) be neutral (because it is a strong acid-strong base salt) d) not be known (because it is a weak acid-weak base salt) e) no correct response
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion O water sodium ion O acetate ion When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion water O sodium ion acetate non aer 20191121-WA0036.jpg Question 9 If the pH of a salt solution is 5.3, the salt must be...
During the titration the following reaction occurs HA + NaOH = NaA+H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? M Use [A] and the pH at the equivalence point to estimate Ko of the weak acid (this is the hard way of estimating K.) Use the pH at the half-way point to estimate of the weak acid (this is the easier way) Your grade will be shown after clicking 'Grade'...
Acid base equalibria
Solution E is made by mixing 1o mL NaA stock solution. e. .H stk solution and 10 .c ml Calculate the [HA]o by dilution of the HA stock solution. Calculate (AJ, by dilution of the NaA stock solution. Calculate [H'Je from the pli. 53 25 From the stoichiometry calculate [A]eq and [HAI Using the values above, calculate K, for the weak acid HA. f. Solution F is made by mixing 2.00 mL HA stock solution and 2o...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
questions are in red
Consider the following salt solutions: (i) NH4Cl – NH+ + C- Notice that as a salt, NH,Cl dissociates completely in solution. So, what are the parents of this salt? The cation, NH, in this case, is from the base obtained by adding enough OHto balance the positive charge(s) on the cation; Viz, NH,OH. Similarly, the anion, Cl. comes from the acid. So the parent acid can be obtained by adding enough Hi to neutralize the charge...
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