Help! Quicklyyyy! Easy science thing.

Which compound contains both ionic and covalent

musickatia [10]

Answer:

(3) NaNO₃

Step-by-step explanation:

Sodium nitrate has ionic bonds, because it consists of Na⁺ and NO₃⁻ ions.

However, the nitrate ions have covalent bonds between the O atoms and the central N atoms.

(1) and (2) are wrong. Both N₂O₅ and HCl consist of nonmetals, so they are covalent compounds.

(4) is wrong. NaCl has only ionic bonds between the Na⁺ and Cl⁻ ions

7 0

3 years ago

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Who invented Microscope

Anit [1.1K]

Answer:

Zacharias Janssen

3 0

3 years ago

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(a) a 0.2 m potassium hydroxide solution is titrated with a 0.1 m nitric acid solution. (i) balanced equation: (ii)what would be

Stells [14]

$\text{KOH} (aq) + \text{HNO}_3 (aq) \to \text{KNO}_3 (aq) + \text{H}_2\text{O} (l)$

The solution shall contain only $\text{KNO}_3 (aq)$ (and water) at the equivalence point. Both potassium hydroxide and nitric acid exist as strong electrolytes. As a result, $\text{KNO}_3 (aq)$ , the salt derived from a reaction between the two species would undergo hydrolysis of a negligible extent. This neutralization reaction therefore be neutral at the equilibrium point.

The question states that the solution is "titrated with a ... nitric acid solution" indicating that $\text{HNO}_3$ is added to the initially-basic solution. PH value of the solution would keep decreasing as the volume of the acid added increases. The final solution would be acidic as it contains not only water and $\text{KNO}_3 (aq)$ , but some $\text{HNO}_3$ as well. Bromothymol blue would therefore demonstrates a yellow color, the color it present in an acidic solution, at the end of the titration.

5 0

3 years ago

A buffer solution is composed of 1.00 mol of acid and 2.25 mol of the conjugate base. If the p K a of the acid is 4.90 , what is

Gemiola [76]

Answer: The pH of the buffer is 5.25

Explanation:

Let the volume of buffer solution be V

We know that:

$\text{Molarity}=\frac{\text{Moles of solute}}{\text{Volume of solution}}$

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

$pH=pK_a+\log(\frac{[\text{conjugate base}]}{[acid]})$

We are given:

$pK_a$ = negative logarithm of acid dissociation constant of weak acid = 4.90

$[\text{conjugate base}]=\frac{2.25}{V}$

$[acid]=\frac{1.00}{V}$

pH = ?

Putting values in above equation, we get:

$pH=4.90+\log(\frac{2.25/V}{1.00/V})\\\\pH=5.25$

Hence, the pH of the buffer is 5.25

4 0

3 years ago

A reaction that occurs in the internal combustion engine is N₂(g) + O₂(g) ⇄ 2NO(g) (c) What is the significance of the different

vodomira [7]

The response would become spontaneous if the value of ΔG° was negative.

According to the estimated value of ΔG°, it is shown that ΔG° value decreases as temperature value increases. The value shifts from being more favorable to being less favorable. It would appear that the value of ΔG° would be negative at a specific temperature, causing the reaction to occur spontaneously.

The reaction is in an equilibrium state if ΔG = 0. If ΔG < 0, the reaction is spontaneous in the direction written. The relationship between terms from the equilibrium is paralleled by the relevance of the sign of a change in the Gibbs free energy.

Learn more about ΔG° here:

brainly.com/question/14512088

#SPJ4

8 0

1 year ago