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NO3-
6.4 x 10-9
MgCl2 aq plus Zn s is the oxidation half-reaction for Mg s plus ZnCl2 aq.
It is the zinc that gets reduced, and the magnesium that gets oxidised. This is because zinc has the higher reduction potential of -0,76 V, compared to magnesiums -2,37 V. The oxidation half cell therefore becomes Mg (s) --> Mg2++ 2e-
Type your answer here... Al(s) | Al3+(aq) Mg2+ (aq) | Mg(s)
they cannot bond together, they are separate .
The Ca2+ ion is larger than the Mg2+ ion. The ionic radii are: 86pm for the Mg2+ and 114pm for the Ca2+. Besides the fact that the Ca2+ has more electrons this can be explained by the principle of electron shielding. Electron shielding is when lower level electrons block the EFC(effective nuclear charge) from effecting the valence electrons of an ion. Ca2+has more electrons than Mg2+ so more electron shielding occurs.
Ca2+ , Mg2+ .
Many metal ions (eg. Ca and Mg) only react completely when EDTA is in pure anionic form (EDTA)4- anion. Since it is a quadruple acid this can only be realized at pH value above 10 for Ca2+ ions, for Mg2+ even higher: >12
Mg is in period 3. Ca is in period 4. Down a group the size increases. So Mg is smaller than Ca.
Total hardness=(Ca2+)*(combining weight of CaCO3/combining weight of Ca2+) +(Mg2+)(combining weight of CaCO3/combining weight of Mg2+)
When Borax is added to water, it reacts with Ca2+ and Mg2+, which come out of water as precipitates. The reactions involved are: Ca2+ + Na2B4O7 ----> CaB4O7 + 2Na+ Mg2+ + Na2B4O7 -----> MgB4O7 + 2Na+
When Borax is added to water, it reacts with Ca2+ and Mg2+, which come out of water as precipitates. The reactions involved are: Ca2+ + Na2B4O7 ----> CaB4O7 + 2Na+ Mg2+ + Na2B4O7 -----> MgB4O7 + 2Na+
Cations are positively charged ions. •Na+ •K+ •Ca2+ •Mg2+
Mg2+ and Ca2+ (and many more!)
CaCO3 calcium carbonate
•Na+, K+, Mg2+, Ca2+, SO42-, Cl-, NO3-, HCO3-