How are the hydrogen atom and lithium atom similar?

If an object is not moving, it has no

Tanzania [10]

Answer:

that answer is B

Explanation:

the answer is b luv

5 0

4 years ago

Read 2 more answers

The ph of a 0. 102 m solution of a weak acid (ha) is 1. 15 ka for the weak acid is?

Advocard [28]

The pH of the weak acid is 6.93.

Given,

K= 1.15 * $10^{-6}$

c=0.102

[H]= K*c= 1.15 * $10^{-6}$ * 0.102= 0.1173 * $10^{-6}$

p[H]= -log[H]= 6.93

A weak acid is one that partially separates into its ions in water or an aqueous solution. A strong acid, on the other hand, completely splits into its ions in water. The conjugate base of a weak acid is also a weak base, and vice versa for the conjugate acid of a weak base. Weak acids have a higher pH than strong acids at the same concentration. Simple arrows pointing left to right are used to represent the reaction of a strong acid ionising in water. On the other hand, a weak acid ionising in water has a double arrow reaction arrow, indicating that both the forward and reverse reactions take place at equilibrium.

Learn more about Weak acid here:

brainly.com/question/22104949

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6 0

1 year ago

A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1a

Vinvika [58]

Explanation:

It is known that relation between $E_{cell}$ , $E^{o}_{cell}$ , and pH is as follows.

$E_{cell} = E^{o}_{cell} - (\frac{0.0591}{n}) \times log[H^{+}]
$

Also, it is known that $E^{o}_{cell}$ for hydrogen is equal to zero.

Hence, substituting the given values into the above equation as follows.

$E_{cell} = E^{o}_{cell} - (\frac{0.0591}{n}) \times log[H^{+}]
$

0.238 V = 0 - (\frac{0.0591}{1}) \times log[H^{+}] [/tex]

$-log[H^{+}]$ = 4.03

$[H^{+}]$ = antilog 4.03

= 3.5

As, pH = $-log[H^{+}]$ .

Thus, we can conclude that pH of the given unknown solution at 298 K is 3.5.

4 0

3 years ago

Calculate the mass of each sample.

Vsevolod [243]

1 mole of any substance has Avagadro number of molecules and it's weight is equal to its molecular weight.
.......................................................................................................................
Answer 1:
Molecular weight of HNO3 = 63.01 g/mol

Therefore, 1mole of HNO3 = 63.03 g
Hence, 15.7 mole of HNO3 = 63.03 X 15.7
= 989.57 g

Thus, mass of 15.7 mole of HNO3 = 989.57 g
..........................................................................................................................
Answer 2:
Molecular weight of H2O2 = 34.01 g/mol

Therefore, 1mole of H2O2 = 34.01g
Hence, 0.00104 mole of H2O2 = 34.01 X 0.00104
= 0.03537 g

Thus, mass of 0.00104 mole of H2O2 is 0.03537 g
.........................................................................................................................
Answer 3:
Molecular weight of SO2 = 64.07 g/mol

Therefore, 1mole of SO2 = 64.07 g
Hence, 72.1 mmole of SO2 = 64.07 X 0.0721
= 4.619 g

Thus, mass of 72.1 mm of SO2 is 4.619 g
.........................................................................................................................
Answer 4:
Molecular weight of XeF2 = 169.29 g/mol

Therefore, 1mole of XeF2 = 169.29 g
Hence, 1.23 mole of XeF2 = 169.29 X 1.23
= 208.23 g

Thus, mass of 1.23 mole of XeF2 is 208.23 g

8 0

4 years ago

how could you check that when the calcium carbonate is reacting with hydrochloric acid the gas given off is carbon dioxide

pav-90 [236]

Answer:

CaCO3 + 2 HCl => CaCl2 + CO2 + H2O

Explanation:

CO2 will burst out when the reaction occurs in water, and the ions will be dissociated: Ca(2+) + 2 Cl (-)

7 0

3 years ago