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Show the equation of dissociation water?
The equation for the dissociation of water is: H2O ↔ H+ + OH-
What is the complete ionic equation for NaOH(aq) plus HCl(aq) H2O() plus NaCl(aq)?
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
What happends to the OH- as the H plus increases?
The concentration of OH- decreases as the concentration of H+ increases. This is beacause there is an equilibrium H2O <-> H+ + OH- and therefore the [H+][OH-] is a constant
Does the dissociation of water produce equal masses of OH- and H plus?
Yes, the dissociation of water produces equal amounts of hydroxide ions (OH⁻) and hydrogen ions (H⁺). The chemical equation for this reaction is ( 2H_2O \leftrightarrow H_3O^+ + OH^- ). For every molecule of water that dissociates, one H⁺ and one OH⁻ ion are generated, resulting in equal concentrations of both ions in pure water at equilibrium.
The equation of combustion of the isopropyl alcohol is C3H7OH I plus O2 g CO2 g plus H2O g How many moles of isopropyl alcohol are required to consume entirely 16 moles of oxygen?
The balanced equation for the combustion of isopropyl alcohol (C₃H₇OH) is: [ C₃H₇OH + 4 O₂ \rightarrow 3 CO₂ + 3 H₂O. ] From the equation, 1 mole of isopropyl alcohol reacts with 4 moles of oxygen. Therefore, to consume 16 moles of oxygen, you would need: [ \frac{16 \text{ moles O₂}}{4 \text{ moles O₂/mole C₃H₇OH}} = 4 \text{ moles of C₃H₇OH}. ] Thus, 4 moles of isopropyl alcohol are required to react with 16 moles of oxygen.
What is the net ionic equation of Na plus plus OH- plus H plus plus Cl- H2O plus Na plus plus Cl-?
The net ionic equation for the given reaction is H+ (aq) + OH- (aq) → H2O (l)
What is H plus and OH?
Water , This is a poorly written chemical equation for the formation/dissociation of water. H^(+) + OH^(-) H2O(l)
What is the complete ionic equation for NaOHaq plus HCIaq equals H2OI plus NaCIaq?
Na+ plus OH- plus H+ equals H2O plus Na+ plus Cl-
Show the equation of dissociation water?
The equation for the dissociation of water is: H2O ↔ H+ + OH-
What is the complete ionic equation for NaOH(aq) plus HCL(aq) H2O(I) plus NaCL(aq)?
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
What is the equation for calculating the change in enthalpy of a system during a chemical reaction?
The equation for calculating the change in enthalpy of a system during a chemical reaction is H H(products) - H(reactants), where H represents the change in enthalpy, H(products) is the enthalpy of the products, and H(reactants) is the enthalpy of the reactants.
Which ion is donated by an acid when added to water OH- OH plus H- or H plus?
H+ or a proton.
What is the equation for calculating frequency?
Frequency F = h/energy = c/wavelength
H plus Cl- plus Na plus OH- Na plus Cl- plus H2O is?
Hydrochloric acid and sodium hydroxide yield salt and water H+ + Cl- + Na+ + OH- --> Na+ + Cl- + H2OComment:In solutions you better leave unchanged ions ( Cl- and Na+) out of the balanced equation: called to be 'tribune ions' (people on the tribune don't take part in the 'match'):H+ + OH- --> H2O This looks simpler than: H+ + Cl - + Na + + OH- --> Na + + Cl - + H2O
What is the complete ionic equation for NaOH(aq) plus HCl(aq) H2O() plus NaCl(aq)?
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
What is the net ionic equation for NaOH plus HCl?
The net ionic equation for the reaction between NaOH and HCl is: OH- + H+ --> H2O. This equation represents the formation of water from the combination of hydroxide ions and hydrogen ions. Sodium and chloride ions are spectators in this reaction and are not involved in the formation of the products.
What is the net ionic equation oh 2H plus plus SO4- plus CA2 plus plus 2l- CaSO4 plus 2H plus 2l-?
To derive the net ionic equation, we first identify the species involved in the reaction. The complete ionic equation shows that we have 2 H⁺ ions, 1 SO₄²⁻ ion, 1 Ca²⁺ ion, and 2 I⁻ ions. When calcium sulfate (CaSO₄) forms, the net ionic equation simplifies to: Ca²⁺ + SO₄²⁻ → CaSO₄(s). The H⁺ and I⁻ ions are spectator ions and do not appear in the net ionic equation.
