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pochemuha
3 years ago
14

Identify each of these substances as acidic, basic, or neutral. pure water, pH = 7.0 lake water, pH = 6.5 baking soda solution,

pH = 9 soapy water, pH = 12
Chemistry
2 answers:
Alex_Xolod [135]3 years ago
5 0

Answer:

pure water, pH = 7.0 (Neutral)

lake water, pH = 6.5 (Acidic)

baking soda solution, pH = 9 (Alkaline)

soapy water, pH = 12 (Alkaline)

Explanation:

The degree of acidicity or alkalinity of a solution can be determined on a pH meter. A pH below 7 is acidic; a pH of 7 is neutral; a pH value of above 7 is alkaline.

Elan Coil [88]3 years ago
4 0

Answer:

Explanation:

NEUTRAL pure water, pH = 7.0

ACIDIC lake water, pH = 6.5

BASIC baking soda solution, pH = 9

BASIC soapy water, pH = 12

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Substances that are readily combustible or may cause fire through friction
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Answer :

Flammable substances

Explanation :

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For example, <em>methanol</em> is a flammable liquid.

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For the following exothermic reaction, A+B⇌C+D + Heat, if the temperature is increased, the reaction will experience a shift to
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How much heat is evolved in converting 1.00 mol of steam at 155.0 ∘c to ice at -50.0 ∘c? the heat capacity of steam is 2.01 j/(g
Ne4ueva [31]
When the specific heat capacity of the water is 4.18 J/g.°C so, we are going to use this formula to get the heat for cooling three  phases changes from steam to liquid and from liquid to ice (solid) :

when Q = M*C*ΔT 

Q is the heat in J

and M is the mass in gram = 1 mol H2O * 18 g/mol(molar mass) = 18 g

C is the specific heat J/g.°C

ΔT is the change in temperature

Q = Mw *[ ( Csteam * ΔTsteam)+(Cw*ΔTw) + (Cice  * ΔT ice)]

    = 18 g * [(2.01 * (155-100°C)) + (4.18 * (100-0°C)) + (2.09 * (0 - 55 °C))]

∴Q = 7444.8 J

and when we know that the heat of fusion for water = 334J/g

and heat of vaporization for water =  2260J/g


∴Q for the two phases changes = M * (2260+334) 

                                                      = 18 * (2260+334)

                                                      = 46692 J 

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5 0
3 years ago
The pH of a 0.150 molar solution of a weak acid is 4.10. What is the pKa of the acid?
Kamila [148]
Answer: 4.21×10⁻⁸

Explanation:


1) Assume a general equation for the ionization of the weak acid:

Let HA be the weak acid, then the ionization equation is:

HA ⇄ H⁺ + A⁻

2) Then, the expression for the ionization constant is:

Ka = [H⁺][A⁻] / [HA]

There, [H⁺] = [A⁻], and [HA] = 0.150 M (data given)


3) So, you need to determine [H⁺] which you do from the pH.

By definition, pH = - log [H⁺]

And from the data given pH = 4.1


⇒ 4.10 = - log [H⁺] ⇒ [H⁺] = antilog (- 4.10) = 7.94×10⁻⁵

4) Now you have all the values to calculate the expression for Ka:

ka = 7.94×10⁻⁵ × 7.94×10⁻⁵ / 0.150 = 4.21×10⁻⁸
3 0
3 years ago
Read 2 more answers
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