In the reaction H2 + CuO → Cu + H2O, hydrogen reduces copper(II) oxide to copper.

Manganese exhibits the highest oxidation state of +7 in permanganate ion (MnO4-).

The bond angle in H2O is approximately 104.5 degrees due to the bent shape of the molecule caused by the two lone pairs on the oxygen atom.

pOH = 14 - pH = 14 - 11 = 3. [OH-] = 10^-pOH = 10^-3 M.

The conjugate base of H2SO4 is HSO4-, formed when H2SO4 donates a proton (H+).

In a tetrahedral complex, the coordination number is 4, as there are four ligands surrounding the central metal atom.

In an octahedral complex, the coordination number is 6, as there are six ligands surrounding the central metal atom.

In the complex ion [H2O]2+, the coordination number of hydrogen is 2.

In the complex [Ni(H2)6], the coordination number of hydrogen is 6, as there are six hydrogen ligands coordinated to nickel.

The coordination number is determined by the number of ligands attached to the central metal ion. In this case, there are six NH3 ligands, giving a coordination number of 6.

The coordination number of copper in [Cu(NH3)4]SO4 is 4, as it is surrounded by four ammonia ligands.

The coordination number is 6 because there are six cyanide ligands coordinated to the iron ion.

The coordination number is 6 because there are six ammonia ligands coordinated to the cobalt ion.

The coordination number is 6 because there are six ammonia ligands coordinated to the cobalt ion.

The coordination number of [Cu(NH3)4]2+ is 4, as it has four ammonia ligands.

The coordination number of [Ni(CN)4]2- is 4, as it has four cyanide ligands coordinated to the nickel ion.

The coordination number is determined by the number of ligand donor atoms bonded to the central metal ion. In [Co(NH3)6]Cl3, there are six ammonia ligands, giving a coordination number of 6.

In [Cu(NH3)4]SO4, copper is coordinated to four ammonia ligands, giving it a coordination number of 4.

The coordination number of the metal ion in [Co(NH3)6]Cl3 is 6, as it is surrounded by six ammonia ligands.

Hydrogen bonding significantly increases the boiling point of water compared to other similar-sized molecules.

Increasing temperature generally decreases the solubility of gases, including hydrogen, in water.

Increasing the concentration of an acid decreases its pH, as pH is inversely related to the concentration of H+ ions.

Increasing the electronegativity of an atom bonded to hydrogen increases the acidity of the compound.

Increasing the oxidation state of a transition metal generally decreases its ionic radius due to increased nuclear charge.

Increasing the oxidation state of a transition metal generally increases its ability to act as a Lewis acid due to a higher positive charge attracting electron pairs more strongly.

Equivalent weight = molar mass / n, where n = number of H+ ions. Molar mass of H2SO4 = 98 g/mol, n = 2. Therefore, equivalent weight = 98 g / 2 = 49 g.

In phosphoric acid, phosphorus has an oxidation state of +5.

The complex formed is [Fe(SCN)3], where iron(III) ions coordinate with thiocyanate ions.

The formula for the compound formed between hydrogen and sulfur is H2S (hydrogen sulfide).

Phosphoric acid serves as an acidulant, providing a tangy flavor and balancing sweetness in soft drinks.