All categories

2 years ago

What is the oxidation number of pt in k2ptcl6?

1 answer:

4 0

Your compound is $K_{2}PtCl_{6}$ .

Remember that the oxidation numbers in a neutral compound must add up to zero. Cl has an oxidation number of -1 because it is a halogen K has an oxidation number of +1 because it is an alkali metal, which exhibits an oxidation state of +1 in compounds.

Since you have 6 atoms of Cl, you have -1(6) = -6 for the Cl. Since you 2 atoms of K, you have +1(2) = +2 for the K. The oxidation number of Pt must make all the oxidation numbers add up to zero:
+2 + (-6) + oxidation number of Pt = 0
-4 + oxidation number of Pt = 0
Oxidation number of Pt = 4

You might be interested in

Select the correct responses to the questions from the drop-down menus.

MA_775_DIABLO [31]

Answer:

Which wind blows cool air inland during the day? Sea Breeze

Which wind blows cool air toward the sea at night? Land Breeze

Which winds blow steadily from specific directions and over long distances? Global Winds

8 0

2 years ago

Read 2 more answers

BH+ClO4- is a salt formed from the base B (Kb = 1.00e-4) and perchloric acid. It dissociates into BH+, a weak acid, and ClO4-, w

Len [333]

Answer:

The pH of 0.1 M BH⁺ClO₄⁻ solution is 5.44

Explanation:

Given: The base dissociation constant: $K_{b}$ = 1 × 10⁻⁴, Concentration of salt: BH⁺ClO₄⁻ = 0.1 M

Also, water dissociation constant: $K_{w}$ = 1 × 10⁻¹⁴

The acid dissociation constant ( $K_{a}$ ) for the weak acid (BH⁺) can be calculated by the equation:

$K_{a}. K_{b} = K_{w}$

$\Rightarrow K_{a} = \frac{K_{w}}{K_{b}}$

$\Rightarrow K_{a} = \frac{1\times 10^{-14}}{1\times 10^{-4}} = 1\times 10^{-10}$

Now, the acid dissociation reaction for the weak acid (BH⁺) and the initial concentration and concentration at equilibrium is given as:

Reaction involved: BH⁺ + H₂O ⇌ B + H₃O+

Initial: 0.1 M x x

Change: -x +x +x

Equilibrium: 0.1 - x x x

The acid dissociation constant: $K_{a} = \frac{\left [B \right ] \left [H_{3}O^{+}\right ]}{\left [BH^{+} \right ]} = \frac{(x)(x)}{(0.1 - x)} = \frac{x^{2}}{0.1 - x}$

$\Rightarrow K_{a} = \frac{x^{2}}{0.1 - x}$

$\Rightarrow 1\times 10^{-10} = \frac{x^{2}}{0.1 - x}$

$As, x$

$\Rightarrow 0.1 - x = 0.1$

$\therefore 1\times 10^{-10} = \frac{x^{2}}{0.1 }$

$\Rightarrow x^{2} = (1\times 10^{-10})\times 0.1 = 1\times 10^{-11}$

$\Rightarrow x = \sqrt{1\times 10^{-11}} = 3.16 \times 10^{-6}$

Therefore, the concentration of hydrogen ion: x = 3.6 × 10⁻⁶ M

Now, pH = - ㏒ [H⁺] = - ㏒ (3.6 × 10⁻⁶ M) = 5.44

Therefore, the pH of 0.1 M BH⁺ClO₄⁻ solution is 5.44

5 0

1 year ago

How much 2 M HBr is needed to neutralize 380 mL of 0.1 M NH4OH?

Nata [24]

Answer:

19ml

Explanation:

trust me

8 0

1 year ago

For the reaction n2(g) + 2h2(g) â n2h4(l), if the percent yield for this reaction is 77.5%, what is the actual mass of hydrazine

Rudiy27

First calculate the moles of N2 and H2 reacted.

moles N2 = 27.7 g / (28 g/mol) = 0.9893 mol

moles H2 = 4.45 g / (2 g/mol) = 2.225 mol

We can see that N2 is the limiting reactant, therefore we base our calculation from that.

Calculating for mass of N2H4 formed:

mass N2H4 = 0.9893 mol N2 * (1 mole N2H4 / 1 mole N2) * 32 g / mol * 0.775

mass N2H4 = 24.53 grams

7 0

2 years ago

The values used in the scale of pH and pOH are derived from a system designed by ______. Gordonsen Sorenson Curie Dalton

yaroslaw [1]

Sorenson

Explanation:

The values used in the scale of pH and pOH are derived from a system designed by Sorenson. Søren Peter Lauritz Sørensen, a Danish chemist introduced the system of pH and pOH for describing the alkalinity and acidity of substances.

The pH and pOH scale is logarithmic scale that ranks the acidity and bascity of compounds.
pH is the negative logarithm of the concentration of hydrogen/hydroxonium ions in solution i.e

pH = -log₁₀{H⁺]

pOH is the negative log of the concentration of the hydroxyl ions in a solution i.e

pOH = -log₁₀{OH⁻]

Learn more:

calculating pH: brainly.com/question/12985875

pH scale: brainly.com/question/11063271

#learnwithBrainly

3 0

2 years ago