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kow [346]
2 years ago
7

What percent of AgNO3 is silver?

Chemistry
1 answer:
Inga [223]2 years ago
8 0

Answer:

63.499%

Explanation:

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If you push on a wall with 200n with what forth with the wall push back
sweet-ann [11.9K]
According to newtons law every action has a equal reaction therefore it will push back 200n aswell
4 0
3 years ago
What causes water to become denser when it is carried to the poles by surface currents? increased temperature and increased sali
Anarel [89]

Answer:

The answer is decreased temperature and increased salinity

Explanation:

It is what is known as the thermohaline circulation

The thermohaline circulation moves the water slowly. This water moves mainly due to differences in its relative density. Much denser water sinks over water that is less dense. Two factors impact the density of seawater: temperature and salinity.

Cold water is denser than hot water:

-Water cools when it loses heat, it occurs at high latitudes.

-Water is heated when it receives energy from the sun, at low latitudes.

Saltier water is much denser than water that has less salt:

-Sea water becomes salty if the evaporation rate increases.

-Sea water becomes less salty if there is a water inlet over the sea.

3 0
3 years ago
Read 2 more answers
Silver metal can be prepared by reducing its nitrate, AgNO3 with copper according to the following equation:
Lerok [7]

%yield = 88.5%

<h3>Further explanation</h3>

Given

Reaction

Cu(s) + 2 AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

Required

The percent yield

Solution

mol AgNO₃(MW=169,87 g/mol) :

= mass : MW

= 127 : 169.87

= 0.748

mol Ag from equation :

= 2/2 x mol AgNO₃

= 2/2 x 0.748

= 0.748

Mass Ag (theoretical) :

= mol x Ar Ag

= 0.748 x 108

= 80.784

% yield = (actual/theoretical) x 100%

%yield = 71.5/80.784 x 100%

<em>%yield = 88.5%</em>

7 0
2 years ago
For the generic equilibrium HA(aq) ⇌ H+(aq) + A−(aq), which of these statements is true? For the generic equilibrium , which of
timama [110]

<u>Answer:</u> The correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

<u>Explanation:</u>

Common ion effect is defined as the effect which occurs on equilibrium when a common ion (an ion which is already present in the solution) is added to a solution. This effect generally decreases the solubility of a solute.

Equilibrium reaction of HA and KA follows the equation:

HA\rightleftharpoons H^{+}(aq.)+A^{-}(aq.)

KA\rightleftharpoons K^+(aq.)+A^{-}(aq.)

According to Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium will shift in the direction in order to minimize the effect.

In the equilibrium reactions, A^- ion is getting increased on the product side, so the equilibrium will shift in the direction to minimize this effect, which is in the direction of HA.

Thus, the addition of KA will shift the equilibrium in the left direction.

Equilibrium constant depends on the temperature of the system. It does not have any effect on any change of pH.

pH is defined as the negative logarithm of hydrogen ions present in the solution

  • If the solution has high hydrogen ion concentration, then the pH will be low.
  • If the solution has low hydrogen ion concentration, then the pH will be high.

As, the equilibrium is shifting in the left direction, that means concentration of H^+ ions are getting decreases. This will increase the pH of the solution.

Hence, the correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

8 0
3 years ago
How many moles of sodium (Na) are there in a<br> sample of 5.87 x 1024 atoms of sodium?
Leno4ka [110]
9.74x 2351 that's the answer
6 0
3 years ago
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