5.1434 contains 5 significant figures and 4 decimals.
<h3>What is a significant figure?</h3>
All zeros that occur between any two non-zero digits are significant. For example, 108.0097 contains seven significant digits.
Calculation:
5.1234 + 0.033÷ 1.650 = 5.1434
5.1434 contains 5 significant figures and 4 decimals. 5.1434 rounded to 4 sig figs is 5.143, to 3 sig figs is 5.14, and to 2 sig figs is 5.1.
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A conductor & a convection current.
Answer:
Complete ionic: .
Net ionic: .
Explanation:
Start by identifying species that exist as ions. In general, such species include:
- Soluble salts.
- Strong acids and strong bases.
All four species in this particular question are salts. However, only three of them are generally soluble in water: , , and . These three salts will exist as ions:
- Each formula unit will exist as one ion and one ion.
- Each formula unit will exist as one ion and two ions (note the subscript in the formula .)
- Each formula unit will exist as one and two ions.
On the other hand, is generally insoluble in water. This salt will not form ions.
Rewrite the original chemical equation to get the corresponding ionic equation. In this question, rewrite , , and (three soluble salts) as the corresponding ions.
Pay attention to the coefficient of each species. For example, indeed each formula unit will exist as only one ion and one ion. However, because the coefficient of in the original equation is two, alone should correspond to two ions and two ions.
Do not rewrite the salt because it is insoluble.
.
Eliminate ions that are present on both sides of this ionic equation. In this question, such ions include one unit of and two units of . Doing so will give:
.
Simplify the coefficients:
.
0.29 M ammonia + 0.38 M ammonium bromide and 0.22 M hypochlorous acid + 0.18 M hydroiodic acids of aqueous solutions are good buffer systems.
<h3>Buffer Systems:</h3>
A solution that resists pH change when acids or bases are added to it is referred to as a buffer system. Either a weak acid and its salt, or a weak base and its salt, make up buffer systems. The ratio of HX/X- does not considerably alter when an acid or a base is introduced to a buffer.
Solutions known as buffers withstand pH changes when an acid or base is added. A weak base (A) and its conjugate weak acid (HA) are both present in buffers. When a reactive system is in equilibrium, adding a strong electrolyte with one common ion will cause the equilibrium to shift, lowering the concentration of the common ion. Buffers differ from one another in terms of pH range and buffer capacity.
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