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3 years ago

Would you use baking powder to see whether or not it is an acid or a substance? yes/no?

Chemistry

2 answers:

alexandr1967 [171]3 years ago

8 0

Yes you would use it

Zanzabum3 years ago

4 0

Answer:

yes.

Explanation:

If you have a liquid and you want to know if it is acidic, an easy way to tell is to mix in a little baking soda. The baking soda reacts with acids to produce bubbles.

You may be familiar with building a homemade kitchen volcano. You mix vinegar (an acid) with baking soda. It foams up as the baking soda reacts with the acid. This is in essence what you can do to test if a solution is acidic or not. If there is no acid present, the solution will not bubble when you add the baking soda.

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How do you know if the reaction is exothermic

MArishka [77]

Hey there!
Exothermic reactions release heat, causing its temperature to fall. If the reaction is lessening the temperature of the object while releasing all the heat, then you know that the reaction is indeed exothermic. Hope this helps!

5 0

3 years ago

Provide a balanced molecular equation, total ionic, and net ionic equation for sodium phosphate and zinc acetate.

vivado [14]

Answer: Balanced molecular equation :

$2Na_3PO_4(aq)+3(CH_3COO)_2Zn(aq)\rightarrow 6CH_3COONa(aq)+Zn_3(PO_4)_2(s)$

Total ionic equation:

$6Na^+(aq)+3PO_4^{2-}(aq)+6CH_3COO^-(aq)+3Zn^{2+}(aq)\rightarrow 6CH_3COO^-(aq)+6Na^+(aq)+Zn_3(PO_4)_2(s)$

The net ionic equation:

$2PO_4^{3-}(aq)+3Zn^{2+}(aq)\rightarrow Zn_3(PO_4)_2(s)$

Explanation:

Complete ionic equation : In complete ionic equation, all the substances that are strong electrolyte are present in an aqueous state as ions.

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

When sodium phosphate and zinc acetate then it gives zinc phosphate and sodium acetate as product.

The balanced molecular equation will be,

$2Na_3PO_4(aq)+3(CH_3COO)_2Zn(aq)\rightarrow 6CH_3COONa(aq)+Zn_3(PO_4)_2(s)$

The total ionic equation in separated aqueous solution will be,

$6Na^+(aq)+2PO_4^{3-}(aq)+6CH_3COO^-(aq)+3Zn^{2+}(aq)\rightarrow 6CH_3COO^-(aq)+6Na^+(aq)+Zn_3(PO_4)_2(s)$

In this equation, and are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$2PO_4^{3-}(aq)+3Zn^{2+}(aq)\rightarrow Zn_3(PO_4)_2(s)$

5 0

3 years ago

A 100.5 ml intraveneous (iv) solution contains 5.10 g glucose (c6h12o6). what is the molarity of this solution?

Pavlova-9 [17]

Answer is: the molarity of this glucose solution is 0.278 M.
m(C₆H₁₂O₆) = 5.10 g.
n(C₆H₁₂O₆) = m(C₆H₁₂O₆) ÷ M(C₆H₁₂O₆) .
n(C₆H₁₂O₆) = 5.10 g ÷ 180.156 g/mol.
n(C₆H₁₂O₆) = 0.028 mol.
V(solution) = 100.5 mL ÷ 1000 mL/L.
V(solution) = 0.1005 L.
c(C₆H₁₂O₆) = n(C₆H₁₂O₆) ÷ V(solution).
c(C₆H₁₂O₆) = 0.028 mol ÷ 0.1005 L.
c(C₆H₁₂O₆) = 0.278 mol/L.

8 0

3 years ago

Which of the following atoms most easily loses an electron Ba Cl Te C P

solong [7]

Ba! It is a metal and wants to lose 2 electrons ASAP

7 0

4 years ago

Astudent prepareda calibration curve by plotting absorbance of the standards against the [FeSCN2+] molar concentration (M). The

Nuetrik [128]

Answer:

Explanation:

Chemistry 1B Experiment 7

1-3 5.0 1.5 3.5

Part 2: Determining the equilibrium constant.

Label 5 medium-sized test tubes. Table 7.2 shows the amounts of 2.00 × 10–3

Fe(NO3)3 (in 1 M HNO3) solution, 2.00 × 10–3

M KSCN solution, and purified water

that should be added to each tube. Pipet the approximate amount of each solution into

each tube. (Record the exact amount of each solution that you actually add. You will

need to use these actual amounts in your calculations.)

Obtain five separate small pieces of parafilm. Close the top of each test tube with

the parafilm. Mix each solution thoroughly by inverting the test tube several times.

Record your observations.

Measure and record the absorbance of each solution at the 447 nm.

Table 7.2 Composition of solutions for determining the equilibrium constant.

Test Tube

Volume of

2.00 × 10–3

M Fe(NO3)3

in 1 M HNO3 (mL)

Volume of

2.00 × 10–3

M KSCN

(mL)

Volume of

purified water

(mL)

2-1 5.0 1.0 4.0

2-2 5.0 2.0 3.0

2-3 5.0 3.0 2.0

2-4 5.0 4.0 1.0

2-5 5.0 5.0 none

Calculations

Part 1. Graphing the relationship between absorbance and [FeSCN2+].

Assuming that “all” of the SCN–

ions have been converted to FeSCN2+ ions,

calculate [FeSCN2+] in each of the solutions in Part 1. For example, in test tube 1-2, 1.0

mL of a 2.00 × 10–3

M KSCN solution was diluted to 10.0 mL. The concentration of

SCN–

that results from this dilution is the one to use for determining [FeSCN2+].

Because of the 1:1 stoichiometry, that initial concentration of SCN– is equal to

[FeSCN2+].

Plot a full-page graph of the absorbance against the concentration of FeSCN2+ in

all standard solutions. Use a ruler to draw the best straight line that comes closest to each

of your five data points. Your line should pass through (0 M, 0). (Why?) This graph is

your calibration curve. When you measure the absorbance of a solution that contains an

unknown concentration of FeSCN2+ ions, you can use this calibration curve to determine

the unknown concentration

6 0

4 years ago