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Arisa [49]
2 years ago
5

Which area is most likely closest to a salt marsh or an estuary?

Chemistry
1 answer:
Archy [21]2 years ago
4 0

Answer:

coastal area with very high tides deep ocean water miles from a river's mouth

Explanation:

Marshes are a type of wetland ecosystem where water covers the ground for long periods of time. Marshes are dominated by herbaceous plants, such as grasses, reeds, and sedges(National Geographic Society).

hope dis help

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Yanka [14]
Because when you take the sand out it doesn't stay the same shape
3 0
3 years ago
Caculate the number if moles of the following: 800. g of Ca
Maru [420]
Mole   is  equal  to   mass  of  the  element  divided  by   molar  mass  of  the  element.  that   is
mole=mass/molar  mass
From  periodic  table calcium  has  a   molar  mass  of  40   g/mol
moles  is   therefore  =800g/40g/mol=20moles
3 0
2 years ago
For 100.0 mL of a solution that is 0.040M CH3COOH and 0.010 M CH3COO, what would be the pH after adding 10.0 mL 50.0 mM HCl?
damaskus [11]

Answer:

The pH of the buffer is 3.90

Explanation:

The mixture of a weak acid CH3COOH and its conjugate base CH3COO produce a buffer that follows the equation:

pH = pKa + log [A-] / [HA]

<em>Where pH is the pH of the buffer, pKa is the pKa of acetic acid (4.75), and [A-] could be taken as the moles of the conjugate base and [HA] the moles of thw weak acid.</em>

<em />

To solve this question we need to find the moles of the CH3COOH and CH3COO- after the reaction with HCl:

CH3COO- + HCl → CH3COOH + Cl-

<em>The moles of CH3COO- are its initial moles - the moles of HCl added</em>

<em>And moles of CH3COOH are its initial moles + moles HCl added</em>

<em />

Moles CH3COO-:

Initial moles  = 0.100L * (0.010mol / L) = 0.00100moles

Moles HCl = 0.010L * (0.050mol / L) = 0.000500 moles

Moles CH3COO- = 0.000500 moles

Moles CH3COOH:

Initial moles  = 0.100L * (0.040mol / L) = 0.00400moles

Moles HCl = 0.010L * (0.050mol / L) = 0.000500 moles

Moles CH3COO- = 0.003500 moles

pH is:

pH = 4.75 + log [0.000500] / [0.00350]

<em>pH = 3.90</em>

<em />

<h3>The pH of the buffer is 3.90</h3>
3 0
3 years ago
Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. suppose we react 7.43 mol calcium with 4.00
Natali [406]
The balanced chemical equation for the above reaction is as follows;
2Ca + O₂ --> 2CaO
stoichiometry of Ca to O₂ is 2:1
this means that 2 mol of Ca reacts with 1 mol of O₂.
If O₂ is the limiting reactant, 
4 mol of O₂ should react with (4x2) - 8 mol of Ca
however only 7.43 mol of Ca is present. Therefore Ca is the limiting reactant.
7.43 mol of Ca reacts with - 7.43/2 = 3.715 mol of O₂
therefore there's excess O₂₂ remaining after the reaction
Since Ca is the limiting reactant, it is fully used up in the reaction and there is no Ca remaining after the reaction is completed.


4 0
2 years ago
I really need help with these three questions PLUS 32 PONITS
raketka [301]
1, neutralization of hydrochloric acid with sodium hydroxide 
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<span>products are water and sodium chloride, also called table salt</span>
8 0
3 years ago
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