Answer:
13.5g of AgNO3 will be needed
Explanation:
Silver nitrate, AgNO3 contains 1 mole of silver, Ag, per mole of nitrate. To solve this problem we need to convert the mass of Ag to moles. Thee moles = Moles of AgNO3 we need. With the molar mass of AgNO3 we can find the needed mass:
<em>Moles Ag-Molar mass: 107.8682g/mol-</em>
8.6g * (1mol / 107.8682g) = 0.0797 moles Ag = Moles AgNO3
<em>Mass AgNO3 -Molar mass: 169.87g/mol-</em>
0.0797 moles Ag * (169.87g/mol) =
<h3>13.5g of AgNO3 will be needed</h3>
Answer:
by pumping blood throughout the body.
Explanation:
Answer:
The answer to your question is Na₂S, if you need to choices the other one is BaS
Explanation:
As a general rule, all the compounds that have sulfur, are insoluble in water, but the are some exceptions.
-Molecules with ammonia
-If the molecule has alkali metals is soluble
-If the molecule has Ca⁺², Sr⁺² and Ba⁺² is soluble in water.
From the compounds given, following the rules, the compound that is soluble in is Na₂S and perhaps BaS.
Answer: The bookkeeper makes cash deposits and records journal entries related to cash, while the treasurer prepares the bank reconciliation.
Explanation: The bookkeeper in an organization is the person in charge of records keeping, his basic task is to keep financial records and therefore the bookkeeper has no business handling physical cash in an organization.
The financial secretary on the hand is in charge saving cash income and withdrawal of cash from an organization, this is done with the organization's accountant approval.
Explanation:
Very little to no formation of silver sulfate, as the silver sulfate Ksp( solubility product) is very large compared to the yellow precipitate Ksp.
By adding sodium sulfate to the silver / yellow precipitate mix, this question asks us to find a potential result and justification for the outcome. This implies that we will have to select the right answer that has a valid result and an adequate explanation for it. A substance's Ksp, or solubility product, is defined as the product of the dissolved ion concentration of each substance elevated to the power of its stoichiometric coefficient.
