You have two aqueous solutions, (1) and (2), at 45°C. Fill in the missing values for each of these solutions in the table below. (At 45°C, the ion-product constant for water is 3.94x10-14, pK, = 13.405.) pH pOH [H,o+] (M) [OH-] (M) (1) 5.50 (2) 4.2x10-10 Step 1 of 10 Write the equation that defines pH in terms of the concentration of hydronium (or hydrogen) ions. The pH of a solution is given by the following equation. O pH = log[H,0*] O pH = In[H;0* ] O pH = -In[H,0* ] -log[H;0+ ] OpH = In this equation [H,0+] is the molar concentration of H,0+ ions. Step 2 of 10 Write the equation that defines pOH in terms of the concentration of hydroxide ions. The pOH of a solution is given by the following equation. O pOH = In[OH- ] O pOH = log[OH ] O pOH = -In[OH¯] PPOH = -log[OH-] In this equation [OH-] is the molar concentration of OH- ions. Step 3 of 10 Write the equation that defines the ion-product constant for water in terms of the concentrations of hydronium ions and hydroxide ions. The ion-product constant for water (K) is given by the following equation. (Equilibrium expressions take the general form: Ke = [C]° / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad Help Greek -
You have two aqueous solutions, (1) and (2), at 45°C. Fill in the missing values for each of these solutions in the table below. (At 45°C, the ion-product constant for water is 3.94x10-14, pK, = 13.405.) pH pOH [H,o+] (M) [OH-] (M) (1) 5.50 (2) 4.2x10-10 Step 1 of 10 Write the equation that defines pH in terms of the concentration of hydronium (or hydrogen) ions. The pH of a solution is given by the following equation. O pH = log[H,0*] O pH = In[H;0* ] O pH = -In[H,0* ] -log[H;0+ ] OpH = In this equation [H,0+] is the molar concentration of H,0+ ions. Step 2 of 10 Write the equation that defines pOH in terms of the concentration of hydroxide ions. The pOH of a solution is given by the following equation. O pOH = In[OH- ] O pOH = log[OH ] O pOH = -In[OH¯] PPOH = -log[OH-] In this equation [OH-] is the molar concentration of OH- ions. Step 3 of 10 Write the equation that defines the ion-product constant for water in terms of the concentrations of hydronium ions and hydroxide ions. The ion-product constant for water (K) is given by the following equation. (Equilibrium expressions take the general form: Ke = [C]° / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad Help Greek -
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Question
 [OH-] (M)
(1) 5.50
(2)
4.2x10-10
Step 1 of 10
Write the equation that defines pH in terms of the concentration of hydronium (or hydrogen) ions.
The pH of a solution is given by the following equation.
pH =
log[H,0+ ]
pH =
In[H,0* ]
pH =
-In[H,0+ ]
O pH =
-log[H,0+ ]
In this equation [H,0+] is the molar concentration of H,o+ ions.
Step 2 of 10
Write the equation that defines pOH in terms of the concentration of hydroxide ions.
The pOH of a solution is given by the following equation.
pOH = In[OH- ]
pOH = log[OH- ]
pOH =
-In[OH- ]
O pOH =
-log[OH- ]
In this equation [OH-] is the molar concentration of OH- ions.
Step 3 of 10
Write the equation that defines the ion-product constant for water in terms of the concentrations of
hydronium ions and hydroxide ions.
The ion-product constant for water (K) is given by the following equation. (Equilibrium expressions take the
general form: Kea
[C] / [A]a . [B]º. Subscripts and superscripts that include letters must be enclosed in
braces {}.)
chemPad
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Greek](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1593f45e-4da7-40d4-bc81-735ecba0bfae%2F571f8a1c-31d0-4b7f-af19-e727e808a13d%2Fkrj8kal_processed.jpeg&w=3840&q=75)
Transcribed Image Text:You have two aqueous solutions, (1) and (2), at 45°C. Fill in the missing values for each of these solutions in
the table below. (At 45°C, the ion-product constant for water is 3.94x10-14, pK
13.405.)
=
pH pOH [H,0*](M) [OH-] (M)
(1) 5.50
(2)
4.2x10-10
Step 1 of 10
Write the equation that defines pH in terms of the concentration of hydronium (or hydrogen) ions.
The pH of a solution is given by the following equation.
pH =
log[H,0+ ]
pH =
In[H,0* ]
pH =
-In[H,0+ ]
O pH =
-log[H,0+ ]
In this equation [H,0+] is the molar concentration of H,o+ ions.
Step 2 of 10
Write the equation that defines pOH in terms of the concentration of hydroxide ions.
The pOH of a solution is given by the following equation.
pOH = In[OH- ]
pOH = log[OH- ]
pOH =
-In[OH- ]
O pOH =
-log[OH- ]
In this equation [OH-] is the molar concentration of OH- ions.
Step 3 of 10
Write the equation that defines the ion-product constant for water in terms of the concentrations of
hydronium ions and hydroxide ions.
The ion-product constant for water (K) is given by the following equation. (Equilibrium expressions take the
general form: Kea
[C] / [A]a . [B]º. Subscripts and superscripts that include letters must be enclosed in
braces {}.)
chemPad
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