Given the following balanced equation , if 5.00 moles of hydrogen gas and 5.00 miles
The concentration of the sulfuric acid : 0.499 M
The net ionic equation
2
OH
⁻(aq]+
2
H
⁺
(aq]
→
2
H
₂O
(l]
<h3>Further explanation</h3>
Given
42.68 ml of 0.43 M KOH
18.40 ml of H2SO4
Required
the concentration of the sulfuric acid
the net ionic equation
Solution
Acid-base titration formula
Ma. Va. na = Mb. Vb. nb
Ma, Mb = acid base concentration
Va, Vb = acid base volume
na, nb = acid base valence
Input the value :
a=KOH, b= H2SO4
0.43 x 42.68 x 1 = Mb x 18.40 x 2
Mb = 0.499 M
The net ionic equation
Reaction
2KOH + H2SO4 → K2SO4 + 2H2O
2
K
⁺
(aq]+
2
OH
⁻
(aq]
+
2
H
⁺
(aq]
+
SO
₄²⁻(aq]
→
2
K
⁺
(aq]
+
SO
₄²⁻(aq]
+
2
H
₂
O
(l]
canceled the spectator ions :
2
OH
⁻(aq]+
2
H
⁺
(aq]
→
2
H
₂O
(l]
Answer:
so I will answer the first question: so if the waning gibbous happened on July 1 then you would expect the waxing crescent.
There are 3 atoms in CO2 (Carbon dioxide).
Carbon has 1 atom and oxygen has 2 atoms.
Answer:
Kp = (Partial pressure H₂O) . (Partial Pressure Cl₂)² / Partial pressure O₂ . (Partial Pressure HCl)⁴
Explanation:
This is the reaction:
4 HCl (g) + O₂ (g) ⇒ 2 Cl₂ (g) + 2 H₂O(g)
Kp = (Partial pressure H₂O) . (Partial Pressure Cl₂)² / Partial pressure O₂ . (Partial Pressure HCl)⁴
