1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
nikklg [1K]
3 years ago
9

Can someone plz help me with this plz?????

Chemistry
1 answer:
Otrada [13]3 years ago
4 0

Answer:

We can't see the options so we don't know what we can put

Explanation:

You might be interested in
Imagine that you're able to fully dissolve a powdered substance in water. what can be said about this creation
ehidna [41]
<span>the water is the solvent, and the powder is the solute. This is also a solution altogether. </span>
8 0
3 years ago
A 31.3-g sample of ammonium carbonate contains ________ mol of ammonium ions.
Leona [35]
<span>We need to calculate the equivalent amount in units of moles of ammonium ions from the mass units. For this we need the molar mass of the substances involved. We calculate as follows: 

31.3 g </span>(NH4)2CO3 ( 1 mol (NH4)2CO3 / 96.09 g (NH4)2CO3) ( 2 mol NH4 / 1 mol (NH4)2CO3 ) = 0.65 mol <span>ammonium ions</span>
7 0
3 years ago
Read 2 more answers
Which elements are more likely to lose electrons?<br> Ca, Li, F and Ne
Slav-nsk [51]
Ca, they only have two valence electrons, in order to become more stable, they would like to lose all of them
3 0
3 years ago
you have been observing an insect that defends itself from enemies by secreting a caustic liquid. analysis of the liquid shows i
Alexus [3.1K]

pH of the buffer solution is 1.76.

Chemical dissociation of formic acid in the water:

HCOOH(aq) ⇄ HCOO⁻(aq) + H⁺(aq)

The solution of formic acid and formate ions is a buffer.

[HCOO⁻] = 0.015 M; equilibrium concentration of formate ions

[HCOOH] + [HCOO⁻] = 1.45 M; sum of concentration of formic acid and formate

[HCOOH] = 1.45 M - 0.015 M

[HCOOH] = 1.435 M; equilibrium concentration of formic acid

pKa = -logKa

pKa = -log 1.8×10⁻⁴ M

pKa = 3.74

Henderson–Hasselbalch equation: pH = pKa + log(cs/ck)

pH = 3.74 + log (0.015 M/1.435 M)

pH = 3.74 - 1.98

pH = 1.76

More about buffer: brainly.com/question/4177791

#SPJ4

4 0
1 year ago
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 17
yawa3891 [41]

Answer:

a. 2 HgO(s) ⇒ 2 Hg(l) + O₂(g)

b. 0.957 g

Explanation:

Step 1: Write the balanced equation

2 HgO(s) ⇒ 2 Hg(l) + O₂(g)

Step 2: Convert 130.0 °C to Kelvin

We will use the following expression.

K = °C + 273.15

K = 130.0°C + 273.15

K = 403.2 K

Step 3: Calculate the moles of O₂

We will use the ideal gas equation.

P × V = n × R × T

n = P × V/R × T

n = 1 atm × 0.0730 L/0.0821 atm.L/mol.K × 403.2 K

n = 2.21 × 10⁻³ mol

Step 4: Calculate the moles of HgO that produced 2.21 × 10⁻³ moles of O₂

The molar ratio of HgO to O₂ is 2:1. The moles of HgO required are 2/1 × 2.21 × 10⁻³ mol = 4.42 × 10⁻³ mol.

Step 5: Calculate the mass corresponding to 4.42 × 10⁻³ moles of HgO

The molar mass of HgO is 216.59 g/mol.

4.42 × 10⁻³ mol × 216.59 g/mol = 0.957 g

5 0
3 years ago
Other questions:
  • How many atoms of each element are present in 3.2 moles of k2so3
    11·2 answers
  • 1 kilogram is the same as 1000 mg
    6·1 answer
  • A liquid that occupies a volume of 9.0 L has a mass of 7.2 kg. What is the density of the liquid in kg/L
    13·1 answer
  • How many grams of calcium are in 3.50 moles of calcium
    11·1 answer
  • From his experiments, J. J. Thomson concluded that
    7·2 answers
  • How many moles of O2 are needed to react completely with 35.0 mol of
    11·1 answer
  • The sun causes water in the pond to evaporate
    9·2 answers
  • The burning of fossil fuels produces what kind of energy​
    13·1 answer
  • Earth's seasons occur due to the tilt of the earth and it's revolution around the sun.
    13·1 answer
  • A sample osoxooso sixisoxoso
    11·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!