Sulfuric acid (H2SO4) reacts with potassium hydroxide (KOH) as follows:
H2SO4(aq) + 2KOH(aq) à K2SO4(aq) + 2H2O(l)
Calculate the volume of 1.00M sulfuric acid required to neutralize 75mL of 0.100M KOH.
H2SO4(aq) + 2KOH(aq) ----------------------------> K2SO4(aq) + 2H2O(l)
C1 = 1.00 M
V1 = ?
n1 = 1
C2 = 0.100 M
V2 = 75 mL
n2 =2
C1 V1 / n1 = C2 V2 / n2
1.00 x V1 / 1 = 0.100 x 75 / 2
V1 = 3.75 mL
volume of H2SO4 = 3.75 mL
H2SO4(aq) + 2KOH(aq) ----------------------------> K2SO4(aq) + 2H2O(l)
C1 = 1.00 M
V1 = ?
n1 = 1
C2 = 0.100 M
V2 = 75 mL
n2 =2
C1 V1 / n1 = C2 V2 / n2
1.00 x V1 / 1 = 0.100 x 75 / 2
V1 = 3.75 mL
volume of H2SO4 = 3.75 mL
Sulfuric acid (H2SO4) reacts with potassium hydroxide (KOH) as follows: H2SO4(aq) + 2KOH(aq) à K2SO4(aq) +...
A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 25.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l)
Deterine the volume of 0.240 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H2SO4(aq)+2KOH(aq)-->K2SO4(aq)+2H2O(L) a) 35mL of 0.240 M H2SO4 b) 175mL of 0.120 M H2SO4 c) 45mL of 0.115 M H2SO4
Determine the volume of 0.220 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H2SO4(aq)+2KOH(aq)→ K2SO4(aq)+2H2O(l) A.45 mL of 0.220 M H2SO4 B.195 mL of 0.120 M H2SO4 C.45 mL of 0.105 M H2SO4
The balanced equation for the neutralization reaction of aqueous H2SO4 with aqueous KOH is shown. H2SO4(aq)+2KOH(aq)⟶2H2O(l)+K2SO4(aq) What volume of 0.130 M KOH is needed to react completely with 11.0 mL of 0.155 M H2SO4?
Determine the volume of 0.230 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H2SO4(aq)+2KOH(aq)→ K2SO4(aq)+2H2O(l)Part A25 mL of 0.230 M H2SO4. Express your answer using two significant figures.
Determine the volume of 0.215 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H2SO4(ag) + 2KOH(aq) → K2So4(aq) + 2H2O(l)Part A 15 mL of 0.215 M H2SO4Part B 185 mL of 0.105 M H2SO4Part C 40 mL of 0.120 M H2SO4
Part A A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 25.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following...
QUESTION 1: A volume of 80.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 12.2 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) QUESTION 2: Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following...
A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 15.2 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)?K2SO4(aq)+2H2O(l) part b: Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents...
Part A A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 19.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Express your answer with the appropriate units. Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a...