Which one of the following statements is true about the neutralization of an acid by a base?
A: The pH decreases when the base is added to the acid. B: Organic compounds are end products. C: Gas is an end product. D: A salt and water are end products
Which of the following is not a correct acid-base neutralization reaction?
The second one needs 2HCl and 2 H20 since it should be CaCl2, as the charge on calcium is 2+ and Cl only has 1- charge, so for the ionic bond, 2 Cl ions are needed
Which of the following statements are true for the reaction HC2H3O2(aq) + KOH(aq) →?
Which of the following statements are true for the reaction HC2H3O2(aq) + KOH(aq) → a) C2H3O2−(aq) is a product b) When balanced the coefficient of KOH(aq) is 1 c) Ions cannot appear in the net ionic equation because they always cancel out on both sides of the equation d) HC2H3O2(aq) appears in the net ionic equation e) OH−(aq) does not appear in the net ionic equation
The following reaction is an acid-base neutralization reaction. True or False?
It's a double replacement reaction so...
Which of the following statements is not true regarding acids?
Acids can be both highly and mildly corrosive. Most fruits contain weak acids. Acids react with bases in neutralization reactions to produce water. Active metals will react with acids in double replacement reactions. Which substance is acting as the Brønsted-Lowry acid in the following chemical reaction? NH4 + OH- ------> NH3 + H2O NH4+? OH- NH3 H2O In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right? 2 SO3 (g) ----> 2 SO2 (g) + O2 (g) H = +197 kJ/mol decrease the temperature increase the volume add more O2 gas add a catalyst
Which of the following is true about double replacement reactions?
In a double-replacement reaction: a) one of the products is always a gas b) one of the products must be an element c) positive ions are exchanged between two compounds d) all of the above Thank you!!
Which of the following statements is correct concerning the neutralization of sulfurous acid by a strong base?
2OH-(aq) + H2SO3(aq) --------------> SO3^2-(aq) + 2H2O(l) a-H2SO3 is an Arrhenius acid, but not a Bronsted-Lowry Acid b-H2SO3 is a Bronsted-Lowry acid, but not an Arrhenius acid c-H2SO3 is both Arrhenius acid and a bronsted-Lowry acid d-H2SO3 is neither an Arrhenius acid nor a Bronsted-Lowry acid e-H2SO3 is a Lewis base
Will HCl or H2SO4 (same concentrations in molarity) require more volume (in mL) to neutralize a solution of NaOH?
All of the other answers here are quite correct, however I thought I’d expand a little bit on the reason why sulphuric acid neutralises twice the molar quantity of NaOH that HCl does. Robert Goodman has hinted at the reason in his answer where he mentions Normality versus Molarity.The reaction of sulphuric acid and sodium hydroxide is normally written as;-H2SO4 + 2 NaOH —→ Na2SO4 + 2H2OFrom this it is clear that one mole of sulphuric acid will neutralise two moles of sodium hydroxide. However the reaction, as written above, is actually the overall reaction resulting from several separate, intermediate reactions.Sulphuric acid is a diprotic acid, which means its ionisation in aqueous solution to produce protons occurs in a two separate stages with the intermediate formation of a bisulphate (or hydrogen sulphate) ion;-H2SO4(l) + H2O(l) —→ H3O+(aq) + HSO4-(aq)HSO4-(aq) + H2O(l) —→ H3O+(aq) + SO4–2(aq)Each reaction releases one mole of hydronium ions (H3O+), each of which can neutralise one mole of NaOH;-H3O+(aq) + OH- (aq) ——-> 2 H2O(l)Similarly, a triprotic acid, such as phosphoric acid (H3PO4), would neutralise three molar equivalents of sodium hydroxide… and so on.