A solution was prepared by mixing 50.00 mL of 0.100 M HNO _{3} and 100.00 mL of 0.200 M HNO_{3}. Calculate the molarity of the final solution of nitric acid.

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Molarity | 23 mins | 0 completed | Learn Summary |

Normality & Equivalent Weight | 24 mins | 0 completed | Learn Summary |

Solution Stoichiometry | 22 mins | 0 completed | Learn |

Solubility Rules | 7 mins | 0 completed | Learn Summary |

Net Ionic Equations | 21 mins | 0 completed | Learn Summary |

Electrolytes | 19 mins | 0 completed | Learn Summary |

Redox Reaction | 32 mins | 0 completed | Learn Summary |

Balancing Redox Reactions | 22 mins | 0 completed | Learn |

Activity Series | 19 mins | 0 completed | Learn |

End of Chapter 4 Problems | 46 mins | 0 completed | Learn |

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Redox Reactions |

Calculate Oxidation Number |

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Dilution |

Net Ionic Equation |

Oxidation Reduction (Redox) Reactions |

Oxidation Number |

Types of Chemical Reactions |

Solution: A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

A solution was prepared by mixing 50.00 mL of 0.100 M HNO _{3} and 100.00 mL of 0.200 M HNO_{3}. Calculate the molarity of the final solution of nitric acid.

When we mix two solutions of differing concentrations, the **final concentration become smaller** than the initial concentration because of dilution resulting from the **increase in total volume**.

We first need to calculate the moles of HNO_{3} in the original solutions. Recall that molarity is:

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